The solution has a total volume of 300 mL and is composed of 100 mL of ethanol (the solute) and 200 mL of water (the solvent).
Does a solution form when 50 mL of ethanol and 50 mL of water are combined?Less than 100 ml will result from mixing 50 ml each of ethanol and water in an equal ratio. This happens because ethanol molecules, which are smaller than those of water, may fit inside big water molecules. As a result, the alcohol content in a 250 mL mix of water and alcohol is 60%.
The combined volumes of the ethanol and water make up the total volume of the solution, which is:
Total volume = 100 mL + 200 mL = 300 mL
Therefore, the solution is made up of 100 mL of ethanol (the solute) and 200 mL of water (the solvent), with a total volume of 300 mL.
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Suppose a skimmer and a gull eat the same fish Over time the skimmer is more successful at catching the fish what would happen to each bird population
Pls help
If a skimmer and a gull eat the same fish and the skimmer is more successful at catching the fish over time, it is likely that the skimmer population would increase, while the gull population may decrease.
What is the skimmer's success in catching the fish?The skimmer's success in catching the fish would give it an advantage in obtaining the necessary nutrients for survival and reproduction. As a result, the skimmer population would likely grow over time as more individuals are able to survive and reproduce due to the abundance of food.
On the other hand, the gull population may decrease due to the competition with the skimmer for the same food source. If the skimmer population grows significantly, it may lead to a reduction in the availability of fish for the gulls to feed on. Over time, this could result in a decline in the gull population due to reduced food availability.
However, it is important to note that the impact on the bird populations may depend on various factors such as the size of the populations, availability of other food sources, and environmental factors. Therefore, the outcome of this scenario cannot be predicted with certainty and would require further analysis and investigation.
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The iodine monobromide molecule, IBr, has a bond length of 249 pm and a dipole moment of 1.21 D. (a) Which atom of the molecule is expected to have a negative charge? (b) Calculate the effective charges on the I and Br atoms in IBr in units of the electronic charge, e.
a. Br will have the negative charge
b. The effective charges on the I and Br atoms are approximately +1.012e and -1.012e, respectively.
How to determine the negative chargea. To identify which atom within an IBr molecule will have a partial negative charge, we must consider each atom's electronegativity.
On the periodic table, iodine (I) has an electronegativity value of 2.66 while bromine (Br) boasts 2.96; since Br has higher electronegativity it will attract electrons more strongly and hence have an even stronger partial negative charge.
B. To calculate the effective charges on the I and Br atoms in IBr, we can use the dipole moment equation:
μ = Q * d
where μ is the dipole moment, Q is the effective charge, and d is the bond length.
We are given the dipole moment (μ) as 1.21 D, and the bond length (d) as 249 pm. However, we need to convert the units to the SI system before proceeding with the calculation.
[tex]1 D (Debye) = 3.336 * 10^-^3^0 cm,\\\\1 pm = 10^-^1^2 m.[/tex]
Now we can solve for the effective charge (Q):[tex]u = 1.21 D * (3.336 × 10^-^3^0 Cm/D)\\ \\= 4.03656 * 10^-^3^0 cm\\d = 249 pm * (10^-12 m/pm) = 2.49 * 10^-^1^0 m[/tex]
Q = μ / d
[tex]Q = (4.03656 * 10^-^3^0 cm) / (2.49 *10^-^1^0 m) \\\\\\=1.62151 * 10^-^2^0 C[/tex]
This effective charge represents the charge difference between the I and Br atoms. To express the charges in units of the elementary charge (e), we need to divide the effective charge by the elementary charge value (e = 1.602 × 10^-19 C):
Q_e =[tex]\frac{(1.62151 * 10^-^2^0 C)}{(1.602 * 10^-^1^9 C)} = 1.012[/tex]
The effective charges on the I and Br atoms are approximately +1.012e and -1.012e, respectively.
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How many grams of NiNO can be produced if 35.1 g of ammonium nitrate and 552 g of sodium phosphate react?
Answer:its b
Explanation:
jusut bcss
Oxygen and oxygen-containing compounds are involved in many different reactions. Which of the following equations represent a balanced reaction involving 14 atoms of oxygen? Question 5 options: NH4Cl + KOH --> NH3 + H2O + KCl 2Na + 2H2O --> 2NaOH + H2 2C2H6 + 7O2 --> 4CO2 + 6H2O 4Fe + 3O2 --> 2Fe2O3
The equation that represents a balanced reaction involving 14 atoms of oxygen is:
2C2H6 + 7O2 --> 4CO2 + 6H2O
a. The relationship between variables in this equation is that 2 moles of C2H6 (ethane) react with 7 moles of O2 (oxygen) to produce 4 moles of CO2 (carbon dioxide) and 6 moles of H2O (water). This equation follows the law of conservation of mass, where the total number of atoms on both sides of the equation is the same, indicating a balanced reaction.
b. The graph is linear, as the coefficients of the reactants and products in the equation are whole numbers and form a consistent ratio. The coefficients of 2, 7, 4, and 6 represent the stoichiometry of the reaction, indicating a fixed relationship between the reactants and products.
c. An example of a situation where this balanced equation could be applicable is the combustion of ethane (C2H6) in the presence of excess oxygen (O2) to produce carbon dioxide (CO2) and water (H2O), which is a common reaction in the combustion of hydrocarbon fuels. The equation represents the balanced stoichiometry of this reaction, where 2 moles of ethane react with 7 moles of oxygen to produce 4 moles of carbon dioxide and 6 moles of water, involving a total of 14 atoms of oxygen in the reaction.
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A 250.0-mL flask contains 0.2500 g of a volatile oxide of nitrogen. The pressure in the flask is 760.0 mmHg at 17.00°C. How many moles of gas are in the flask?
Answer:
0.0104 moles of gas in the flask.
Explanation:
To calculate the number of moles of gas in the flask, you can use the ideal gas law equation: PV = nRT. Where P is pressure, V is volume, n is the number of moles, R is the ideal gas constant and T is temperature.
First, you need to convert the pressure from mmHg to atm and the temperature from Celsius to Kelvin. The pressure in atm is 760.0 mmHg / 760 mmHg/atm = 1 atm. The temperature in Kelvin is 17.00°C + 273.15 = 290.15 K.
Next, you need to convert the volume from mL to L. The volume in L is 250.0 mL / 1000 mL/L = 0.2500 L.
Now you can plug all the values into the ideal gas law equation and solve for n: (1 atm)(0.2500 L) = n(0.08206 L·atm/mol·K)(290.15 K). Solving for n gives n = 0.0104 mol.
So there are approximately 0.0104 moles of gas in the flask.
in an experiment, 1 mol A, 2 mol B and 1 mol D were mixed and allowed to come to equilibrium at 25C. The resulting mixture was found to contain 0.9 mol of C at a total pressure of 1.00 bar. Find the mole fractions of each species at equilibrium
The mole fractions of each species at equilibrium are 0.25 for A and D, 0.5 for B, and 0.225 for C.
we can use the principles of chemical equilibrium and the mole fraction formula.
First, we need to write the balanced chemical equation for the reaction involving A, B, C, and D. Let's assume that the reaction is:
A + 2B <=> C + D
where A, B, C, and D are the chemical species, and the coefficients indicate their stoichiometric ratios.
Next, we need to write the expression for the equilibrium constant, Kc, for this reaction:
Kc = [C][D] / [A][B]²
where [X] denotes the molar concentration of species X at equilibrium.
Since we know the initial moles of A, B, and D, we can calculate their total moles in the mixture:
Total moles = 1 mol A + 2 mol B + 1 mol D = 4 mol
We also know that the final mixture contains 0.9 mol of C. Therefore, the molar concentration of C at equilibrium is:
[C] = 0.9 mol / 4 L = 0.225 M
Since we have only one unknown, we can use the equilibrium constant expression to calculate the molar concentration of D:
Kc = [C][D] / [A][B]²
0.9 = (0.225)(D) / (1)(2²)
D = 1.8
Therefore, the molar concentration of D at equilibrium is 1.8 M.
Using the law of conservation of mass, we can also calculate the molar concentration of A and B at equilibrium:
[A] = 1 mol / 4 L = 0.25 M
[B] = 2 mol / 4 L = 0.5 M
Mole fraction of X = moles of X / total moles
Mole fraction of A = 1 mol / 4 mol = 0.25
Mole fraction of B = 2 mol / 4 mol = 0.5
Mole fraction of C = 0.9 mol / 4 mol = 0.225
Mole fraction of D = 1 mol / 4 mol = 0.25
Therefore, the mole fractions of each species at equilibrium are 0.25 for A and D, 0.5 for B, and 0.225 for C.
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The compounds labeled benzophenone-3 (C14H12O3) and benzophenone-5 (C14H11NaO6S) are found in certain sunscreens. Would you expect a sunscreen made with benzophenone-3 or benzophenone-5 be more waterproof? Explain your choice.
A sunscreen made with Benzophenone-5 ([tex]C_1_4H_1_1NaO_6S[/tex]) would be expected to be more waterproof than benzophenone-3 ([tex]C_1_4H_1_2O_3[/tex]).
This is due to the presence of a sodium salt group (Na) and a sulfonic acid group ([tex]SO_3H[/tex] ) in benzophenone-5, which makes it more polar than benzophenone-3. Polar molecules interact more strongly with water molecules and are less likely to dissolve in nonpolar solvents such as oils.
Because sunscreen is designed to be water-resistant, the more polar benzophenone-5 should have stronger interactions with water and give more water resistance than benzophenone-3.
Moreover, the sulfonic acid group in benzophenone-5 may allow it to make stronger hydrogen bonds with water, increasing its water resistance even further.
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your answer to the following question on the information below and you knowledge of chemistry.
A 100. -gram sample of liquid water is heated from 30.0°C to 80.0°C. Enough KCIO:(s) is dissolved in the sample of water at 80.0°C to form a saturated solution.
Based on Table H, determine the vapor pressure of the water sample at its final temperature.
Explanation:
Table H lists vapor pressure data for pure water at various temperatures. We can use this data to estimate the vapor pressure of the water in the given system at its final temperature of 80.0°C.
First, we need to calculate the heat absorbed by the water sample during the heating process. We can use the specific heat capacity of water to do this:
q = m * c * ΔT
where q is the heat absorbed, m is the mass of water (100 g), c is the specific heat capacity of water, and ΔT is the temperature change (80°C - 30°C = 50°C).
Plugging in the values, we get:
q = 100 g * 4.18 J/(g*C) * 50 C
q = 20900 J
This tells us that 20,900 joules of energy were absorbed by the water sample during heating.
Next, we need to consider the saturated solution of KCIO3 in the water sample. At 80.0°C, the water is already close to boiling, so it is likely that the vapor pressure of the water in the system is close to the vapor pressure of pure water at this temperature. From Table H, we can see that the vapor pressure of pure water is approximately 356 mmHg at 80.0°C.
Therefore, the vapor pressure of the water in the given system at its final temperature of 80.0°C is approximately 356 mmHg.
Calculate the volume of C2H2 that is collected over water at 23 ∘C by a reaction of 1.52 g of CaC2 if the total pressure of the gas is 751 torr. (The vapor pressure of water is 21.07 torr .)
The volume of C₂H₂ that is collected over water at 23 ∘C by the reaction of 1.52 g of CaC₂ is 0.61 L
How do i determine the volume of C₂H₂ collected?First, we shall determine the mole of CaC₂ that reacted. Details below:
Mass of CaC₂ = 1.52 g Molar mass of CaC₂ = 64 g/mol Mole of CaC₂ =?Mole = mass / molar mass
Mole of CaC₂ = 1.52 / 64
Mole of CaC₂ = 0.024 mole
Next, we shall determine the mole of C₂H₂. obtained. Details below:
CaC₂ + 2H₂O -> C₂H₂ + Ca(OH)₂
From the balanced equation above,
1 mole of CaC₂ reacted to produced 1 mole of C₂H₂
Therefore,
0.024 mole of CaC₂ will also react to produce 0.024 mole of C₂H₂
Finally, we shall determine the volume of C₂H₂ collected. This is shown below:
Temperature (T) = 23 °C = 23 + 273 = 296 KVapor pressure = 21.07 torrPressure of dry gas (P) = 751 - 21.07 = 729.93 torrGas constant (R) = 62.36 torr.L/mol KNumber of mole (n) = 0.024 moleVolume of gas (V) =?PV = nRT
729.93 × V = 0.024 × 62.36 × 296
Divide both sides by 729.93
V = (0.024 × 62.36 × 296) / 729.93
V = 0.61 L
Thus, the volume of the C₂H₂ gas collected is 0.61 L
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Chemistry what is the reaction Rate TABLE
The rate constant, k = 5.27 E-2 s⁻¹, determines the rate law for the reaction P → E + Z.
How to determine rate constant?The rate of the reaction P → E + Z can be expressed as:
Rate = - d[P]/dt = d[E]/dt = d[Z]/dt
where d[P], d[E], and d[Z] = changes in the concentrations of P, E, and Z, respectively, over a small time interval dt.
Use the experimental data to determine the rate constant and the order of the reaction.
Calculate the initial rate of the reaction in each trial by dividing the change in concentration of P by the time interval:
rate1 = (d[P]/dt)1 = (0.30 M - 0 M)/(20 s) = 0.015 M/s
rate2 = (d[P]/dt)2 = (0.60 M - 0.30 M)/(20 s) = 0.015 M/s
rate3 = (d[P]/dt)3 = (0.90 M - 0.60 M)/(20 s) = 0.015 M/s
The initial rates are the same in all three trials, which suggests that the reaction is first-order with respect to P.
Now using any of the three trials to determine the value of the rate constant k, trial 1:
Rate1 = k[P]1
k = Rate1/[P]1 = (1.58 E-2 M/s)/(0.30 M) = 5.27 E-2 s⁻¹
Therefore, the rate law for the reaction P → E + Z is:
Rate = k[P]
where k = 5.27 E-2 s⁻¹ is the rate constant.
Use the rate law to calculate the expected rates of the reaction at different concentrations of P. For example:
Rate2 = k[P]2 = (5.27 E-2 s⁻¹)(0.60 M) = 3.16 E-2 M/s
Rate3 = k[P]3 = (5.27 E-2 s⁻¹)(0.90 M) = 4.74 E-2 M/s
These expected rates are close to the experimental rates, which suggests that the rate law is a good approximation for the reaction under these conditions.
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A gas‑filled weather balloon has a volume of 56.0 L
at ground level, where the pressure is 761 mmHg
and the temperature is 23.1 ∘C.
After being released, the balloon rises to an altitude where the temperature is −6.97 ∘C
and the pressure is 0.0772 atm.
What is the weather balloon's volume at the higher altitude?
We can use the combined gas law to determine the volume of the balloon at a higher altitude. The combined gas law relates the pressure, volume, and temperature of a gas:
(P1 x V1) / T1 = (P2 x V2) / T2
where P1, V1, and T1 are the pressure, volume, and temperature of the gas at the initial state, and P2, V2, and T2 are the pressure, volume, and temperature of the gas at the final state.
We are given the initial pressure (P1 = 761 mmHg), volume (V1 = 56.0 L), and temperature (T1 = 23.1 °C = 296.25 K) of the gas, and the final pressure (P2 = 0.0772 atm), and temperature (T2 = -6.97 °C = 266.18 K) of the gas. We can solve for V2, the final volume of the gas:
(P1 x V1) / T1 = (P2 x V2) / T2
V2 = (P1 x V1 x T2) / (P2 x T1)
V2 = (761 mmHg x 56.0 L x 266.18 K) / (0.0772 atm x 296.25 K)
V2 = 2,040 L (rounded to three significant figures)
Therefore, the volume of the weather balloon at the higher altitude is approximately 2,040 L.
add a given instant what is the rate of appearance at this time
The rate of appearance of NOBr at the given time is 9.80 × [tex]10^-^4[/tex] M/s which is the second option as the question asks to determine the rate of appearance of NOBr, which is a product of the given chemical reaction, at the given time when the rate of disappearance of Br₂ is known.
For every 1 mole of Br₂ that disappears, 2 moles of NOBr appear. Thus, we can set up a proportion:
(2 mol NOBr / 1 mol Br₂) = (rate of appearance of NOBr / rate of disappearance of Br₂)
Substituting the given values,
(2 mol NOBr / 1 mol Br₂) = (rate of appearance of NOBr / 4.90 x [tex]10^-^4[/tex] M/s)
Solving for the rate of appearance of NOBr,
rate of appearance of NOBr = (2 mol NOBr / 1 mol Br₂) x (4.90 x [tex]10^-^4[/tex] M/s) = 9.80 × [tex]10^-^4[/tex]M/s
The rate of appearance of NOBr at the given time is 9.80 × [tex]10^-^4[/tex] M/s.
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What is the number of molecules of NO, which contains 16 gm of oxygen. 14
1. Which metal is the most reactive? How do you know this?
2. Rank the metals in order of increasing reactivity.
3. Give the chemical equations for each single replacement reaction that took place.
4. Was Fe^3+ reduced? Of so what metal(s) acted as reducing agents?
What is the molarity of a solution that has 2.0 moles of solute in 3.0 L of solution?
The molarity of the solution that has 2.0 moles of solute in 3.0 L of solution is 0.67 mol/L
What is molarity?Molarity is described as a measure of the concentration of a chemical species, in particular of a solute in a solution, in terms of amount of substance per unit volume of solution.
Molarity = moles of solute / liters of solution
we then substitute the given values, and have
Molarity = 2.0 moles / 3.0 L
Molarity = 0.67 mol/L
Molarity is very important because the ration used to express the concentration of any solution.
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Chemistry..... Reaction Rate
W → U + S Chemistry Reaction Rate use the table to find reaction rate
See reaction Rate Table Picture
The reaction rates for trial 1 is 8.22 x 10⁻² M⁻² s⁻¹ and 1.10 M⁻² s⁻¹ for trail 2 and 3
How to find reaction rate?Keep the concentration of W constant while varying the concentrations of U and S while measuring the reaction rate in order to determine the reaction rate with regard to U and S.
Select trial 1 as the reference trial and calculate the reaction's rate constant (k) with respect to U and S, assuming that the concentration of W is constant throughout all three trials.
For trial 1:
[W] = 0.13 M
Rate = 4.72 x 10⁻⁴ M/s
For trial 2:
[W] = 0.13 M
Rate = 1.18 x 10⁻² M/s
From the equation rate = k[U][S], set up the following ratio of rates:
Rate2/Rate1 = (k[U]2[S]2)/(k[U]1[S]1)
Simplifying:
k = (Rate2/Rate1) x (1/[U]2) x (1/[S]2) x ([U]1) x ([S]1)
Substituting the values from trials 1 and 2:
k = (1.18 x 10⁻² M/s) / (4.72 x 10⁻⁴ M/s) x (1/0.65 M) x (1/1 M) x (0.13 M) x (1 M)
k = 8.22 x 10⁻²M⁻² s⁻¹
Similarly, for trial 3:
[W] = 0.13 M
Rate = 2.95 x 10⁻¹ M/s
Again, using trial 1 as the reference trial, figure out the reaction's rate constant (k) in relation to U and S:
k = (Rate3/Rate1) x (1/[U]3) x (1/[S]3) x ([U]1) x ([S]1)
k = (2.95 x 10⁻¹ M/s) / (4.72 x 10⁻⁴ M/s) x (1/3.25 M) x (1/1 M) x (0.13 M) x (1 M)
k = 1.10 M⁻² s⁻¹
Therefore, the equation states the reaction rate in relation to U and S is k = 8.22 x 10⁻² M⁻² s⁻¹ and 1.10 M⁻² s⁻¹ for trials 2 and 3, respectively.
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how many moles of a salute are needed to prepare 300 mL of 0.8 mm and NACL solution
Answer: 0.24 Moles. WARNING: "mm" in the original question seems to be a typo and was assumed to be "M" (moles per liter) for concentration.
Explanation:
To calculate the number of moles of solute needed to prepare a solution, we can use the formula:
moles of solute = concentration (in moles per liter) * volume of solution (in liters)
Given:
Concentration of NaCl solution = 0.8 M (moles per liter)
Volume of solution to be prepared = 300 mL = 300/1000 L (converted to liters)
Plugging in the given values:
Concentration = 0.8 M
Volume of solution = 300/1000 L
moles of NaCl = 0.8 M * 300/1000 L
Calculating:
moles of NaCl = 0.24 moles
So, 0.24 moles of NaCl are needed to prepare 300 mL of a 0.8 M NaCl solution.
A 0.4856 g sample of solid silver oxide is heated. Find the volume of O2 that can be released at STP.
The volume of O2 that can be released at STP from the given sample of silver oxide is 23.45 mL.
To solve this problem
Creating the balanced chemical equation for the breakdown of silver oxide is the first step in tackling this issue:
2Ag2O(s) → 4Ag(s) + O2(g)
We can deduce from the equation that 2 moles of AgO will result in 1 mole of O2. Since Ag2O has a molar mass of 231.735 g/mol, 0.4856 g of Ag2O is equivalent to:
0.4856 g Ag2O x (1 mol Ag2O/231.735 g Ag2O) = 0.002095 mol Ag2O
Therefore, the number of moles of O2 that can be produced from 0.4856 g of Ag2O is:
0.002095 mol Ag2O x (1 mol O2/2 mol Ag2O) = 0.0010475 mol O2
1 mole of any gas takes up 22.4 L of space at STP As a result, 0.4856 g of Ag2O can generate the following amount of O2 at STP:
0.0010475 mol O2 x 22.4 L/mol = 0.02345 L or 23.45 mL
Therefore, the volume of O2 that can be released at STP from the given sample of silver oxide is 23.45 mL.
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Acetic acid has a molar mass of 60.05 g/mol. If 16.84 grams of acetic acid are present, how many moles of acetic acid does that correspond to?
Answer:
3.566 mol
Explanation:
Since 60.05 is grams divided by mol to cancel out the grams to get only mols it must be divided by 16.84 g
[tex]\frac{60.05 g}{mol} *\frac{1 }{16.84g} =3.566[/tex] mols acetic acid
All redox reactions form ionic bonds. True or False
Answer:
true
Explanation:
Given the following reaction:
2C₂H₂(g) + 5O₂(g) → 4CO₂(g) + 2H₂O(g) ∆H = -2511.6 kJ
What is the energy change when 7.76 g of C₂H₂ react with excess O₂?
Chemical reactions nearly always include a change in energy between the products and reactants.
Thus, Energy is released when chemical bonds are created and is released when chemical bonds are destroyed.
The overall energy of a system, however, must remain constant according to the Law of Conservation of Energy, and chemical reactions frequently absorb or release energy in the form of heat, light, or both.
The difference in the amounts of chemical energy that are stored in the products and reactants accounts for the energy change in a chemical reaction. Enthalpy refers to the system's heat content or stored chemical energy.
Thus, Chemical reactions nearly always include a change in energy between the products and reactants.
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All changes saved
5. The head of matches contains an oxidizing agent such as potassium chlorate, KCIO3, together with tetraphosphorus trisulfide, P4S3.
glass, and binder. When struck either by an obect or on the side of a box of matches, the phosphorus sulfide compound is easily
ignited, causing the potassium chlorate to decompose into potassium chloride and oxygen. The oxygen in turn causes the
phosphorus sulfide to burn more vigorously.
Determine the oxidation number of chlorine in potassium chlorate.
The oxidation number of the unknown chlorine in the compound is + 5
What is oxidation number?The oxidation number of an element in a compound is determined by a set of rules based on its position in the periodic table, as well as the charges of other atoms in the compound
We know that the oxidation number of the chlorine which we want to obtain would be designated as x and the total of the oxidation numbers of the elements in the compound is zero.
Thus we have that;
1 + x + 3(-2) = 0
1 + x - 6 = 0
-5 + x = 0
x = 5
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A specific organic reaction is described by the energy diagram drawn below. Using this
energy diagram, identify which product will form first and which product will be the
major product if given enough time?
The product that is formed first is product B and the product that will be the major product if given enough time would also be product B.
In an energy diagram, the vertical axis represents the overall energy of the reactants, while the horizontal axis is the ‘reaction coordinate’, tracing from left to right the progress of the reaction from starting compounds to final products.
The activation energy of the reaction can be shown on a diagram as the energy between the reactants that the transition state.
The product with lesser activation energy is the product that is formed first and the major product is decided by the stability of the product which depends on the energy. Lesser is the energy of the product, greater is its stability.
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Potassium superoxide, KO2, reacts with carbon dioxide to form potassium carbonate and oxygen:
This reaction makes potassium superoxide useful in a self-contained breathing apparatus. How much O2 could be produced from 2.61 g of KO2 and 4.46 g of CO2?
First, we need to write out the balanced chemical equation for the reaction: 4 KO2 + 2 CO2 → 2 K2CO3 + 3 O2
From the equation, we can see that 4 moles of KO2 react with 2 moles of CO2 to produce 3 moles of O2. Therefore, we need to convert the given masses of KO2 and CO2 into moles:
moles of KO2 = 2.61 g / molar mass of KO2 = 2.61 g / 71.10 g/mol = 0.0367 mol
moles of CO2 = 4.46 g / molar mass of CO2 = 4.46 g / 44.01 g/mol = 0.1013 mol
Next, we need to determine the limiting reagent (the reactant that will be completely consumed in the reaction) by comparing the mole ratios of KO2 and CO2 in the balanced equation. The ratio of moles of KO2 to moles of CO2 is:
0.0367 mol KO2 / 4 mol KO2 per 2 mol CO2 = 0.0184 mol CO2
Since this ratio is less than the actual number of moles of CO2 we have (0.1013 mol), CO2 is in excess and KO2 is the limiting reagent.
Using the mole ratio from the balanced equation, we can calculate the number of moles of O2 produced:
moles of O2 = 3 mol O2 per 4 mol KO2 × 0.0367 mol KO2 = 0.0275 mol O2
Finally, we can convert the moles of O2 to grams:
mass of O2 = moles of O2 × molar mass of O2 = 0.0275 mol × 32.00 g/mol = 0.88 g
Therefore, 2.61 g of KO2 and 4.46 g of CO2 would produce 0.88 g of O2.
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How many grams of Al are needed to react with 352 mL of a 1.65 M HCl solution? Given the equation 2Al + 6HCl yields to form 2AlCl3 + 3H2
5.221 grams of Al are required to react with 352 mL of 1.65 M HCl solution.
What is meant by molarity?Molarity (M) is defined as the moles of solute per liter of the solution.
Balanced chemical equation is : 2Al + 6HCl → 2AlCl₃ + 3H₂
From the equation, we can see that 2 moles of Al react with 6 moles of HCl to produce 2 moles of AlCl₃ and 3 moles of H₂.
As moles of HCl = Molarity × Volume
moles of HCl = 1.65 mol/L × 0.352 L
moles of HCl = 0.58128 mol
and moles of Al = (2/6) × moles of HCl
moles of Al = (1/3) × 0.58128 mol
moles of Al = 0.19376 mol
mass of Al = moles of Al × molar mass of Al
mass of Al = 0.19376 mol × 26.98 g/mol
mass of Al = 5.221 g
So, 5.221 grams of Al are required to react with 352 mL of 1.65 M HCl solution.
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If 12.5 mol
of an ideal gas occupies 50.5 L
at 69.00 ∘C,
what is the pressure of the gas?
The pressure of a gas that occupies 50.5L at 69.0°C is 6.95 atm.
How to calculate pressure?The pressure of an ideal gas can be calculated using Avogadro's equation as follows;
PV = nRT
Where;
P = pressureV = volume n = no of molesT = temperatureR = gas law constantAccording to this question, 12.5 mol of an ideal gas occupies 50.5 L at 69.00°C. The pressure can be calculated as follows:
P × 50.5 = 12.5 × 0.0821 × 342
50.5P = 350.9775
P = 6.95 atm
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What is the molar equilibrium concentration of Cu2+ in a solution where 1.00 L of 0.800 M [Cu(NH3)4]2+ has 0.100 mol NH3 added to it, without any change in volume. The equation is Cu2+(aq) + 4 NH3(aq) [Cu(NH3)4]2+(aq) , where Kf = 2.1 x 1013
The molar equilibrium concentration of Cu² ⁺ is [tex]3.3 x 10^-26[/tex]M when 0.100 mol NH₃ is added to 1.00 L of 0.800 M with Kf = [tex]2.1 x 10^13[/tex].
The issue includes computing the molar balance convergence of Cu² ⁺ in an answer that has 0.100 mol NH3 added to 1.00 L of 0.800 M [Cu(NH₃)₄]²⁺ . To tackle the issue, we can involve the balance consistent articulation for the arrangement of[Cu(NH₃)₄]²⁺:
Kf =[Cu(NH₃)₄]²⁺/(Cu² ⁺)(NH₃)₄
Since the volume of the arrangement doesn't change when NH₃ is added, the underlying grouping of [Cu(NH₃)₄]²⁺ is as yet 0.800 M, while the underlying convergences of Cu² ⁺ and NH₃ are zero. Let x be the molar centralization of Cu² ⁺ at balance, and (0.100 - 4x) be the molar grouping of NH₃ at harmony. Then, we can compose the harmony consistent articulation as:
[tex]2.1 x 10^13 = (x)(0.800 - x)^4/(0.100 - 4x)^4[/tex]
Settling for x gives the molar balance convergence of Cu² ⁺ as 3.3 x [tex]10^-26[/tex] M. This tiny focus demonstrates that the majority of the copper in the arrangement is as [Cu(NH₃)₄]²⁺ and that the expansion of NH₃ has moved the harmony towards the development of this complex.
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What mass of oxygen would be released by the thermal decomposition of 918.7 grams of Mercury (II) Oxide?
HgO --> Hg + O2
Answer:
Explanation:
[tex]\frac{918.7 g}{1} *\frac{1}{216.59m } = 4.241 mol[/tex] To start off the mol of HgO must be found.
After that the molar ratio between HgO and O must be found but in this case its 1:1
[tex]4.241 mol HgO*\frac{1 molO}{1molHgO} = 4.241 mol O[/tex] the mols of HgO is put on the bottom to cancel out with the other one leaving just mols of oxygen. Finally to find g of oxygen it must be multiplied by its molar mass.
[tex]\frac{4.241 molO}{1} * \frac{15.999 g}{mol} = 67.85 g[/tex] Oxygen
HELP PLEASE
A 6.50-g sample of copper metal at 25.0 °C is heated by the addition of 145 J of energy. The final temperature of the copper is ________ °C. The specific heat capacity of copper is 0.38 J/g-K.
58.7
33.7
83.7
25.0
33.5
A 6.50-g sample of copper metal at 25.0 °C is heated by the addition of 145 J of energy. The final temperature of the copper is 83.7 °C. The specific heat capacity of copper is 0.38 J/g-K.
The correct answer choice is "83.7"
To solve this problem, we can use the equation:
q = mcΔT
where q is the amount of energy absorbed by the copper, m is the mass of the copper, c is the specific heat capacity of copper, and ΔT is the change in temperature of the copper.
Rearranging this equation to solve for ΔT, we get:
ΔT = q / (mc)
Substituting the given values, we get:
ΔT = 145 J / (6.50 g x 0.38 J/g-K)
ΔT = 58.7 K
Therefore, the final temperature of the copper is:
25.0 °C + 58.7 °C = 83.7 °C
So the correct option is 83.7.
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If a balloon containing a mixture of gases where the partial pressure of oxygen is 12.8 psi, the partial pressure of hydrogen is 4.31 psi, and the partial pressure of nitrogen is 22.1 psi, then the actual pressure inside the balloon is…
Answer:
39.21 psi
Explanation:
According to Dalton's Law, the total pressure in the system is the sum of all the partial pressures, so all you need to do is add the partial pressures :)
