(a) To calculate the mass of sulfuric acid in the truck, we can multiply the volume of sulfuric acid by its density. Given that the truck carries 34,000 liters of sulfuric acid and the density of sulfuric acid is 1.84 kg/L.
we can use the formula:
Mass (m) = Volume (V) × Density (D)
Plugging in the given values:
Volume (V) = 34,000 L Density (D) = 1.84 kg/L
m = 34,000 L × 1.84 kg/L
m ≈ 62,560 kg (rounded to the nearest whole number)
Therefore, the mass of sulfuric acid in the truck is approximately 62,560 kg.
(b) The amount of sulfuric acid in the truck is already given in the question as 34,000 L (volume).
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(a) To find the mass of sulfuric acid in the truck, we need to use the formula:
mass = density x volume
The volume of sulfuric acid in the truck is given as 34,000 L. The density of sulfuric acid is 1.84 kg/L. Therefore, the mass of sulfuric acid in the truck is:
mass = 1.84 kg/L x 34,000 L = 62,560 kg
So there are 62,560 kg of sulfuric acid in the truck.
(b) To find the amount of sulfuric acid in the truck, we need to use the formula:
amount = mass / molar mass
The molar mass of sulfuric acid is 98.08 g/mol. To convert the mass from kg to g, we need to multiply by 1000. Therefore, the amount of sulfuric acid in the truck is:
amount = 62,560,000 g / 98.08 g/mol = 636,816.3 mol
So there are 636,816.3 moles of sulfuric acid in the truck.
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Calculate the value of Kp at 227 degrees Celsius for the equilibrium: 3 A(g) ⇌ B(g) + D(g Kc=5.15
You perform a reaction in a coffee cup calorimeter. The calorimeter has 100 mL of water in it, and the temperature of the water increases by 9.3°C. The calorimeter has a heat capacity of 50.2 J/°C. How much heat was produced by the reaction (specific heat capacity of water is 4.184 J/g-°C)?
We can use the equation:
q = m * c * ΔT
where q is the heat absorbed or released by the water, m is the mass of water, c is the specific heat capacity of water, and ΔT is the change in temperature of the water.
Since we know that the calorimeter contains 100 mL (or 100 g, since 1 mL of water has a mass of 1 g) of water and that the temperature of the water increased by 9.3°C, we can plug in these values:
q = (100 g) * (4.184 J/g-°C) * (9.3°C)
q = 3896.68 J
However, this is not the total amount of heat produced by the reaction. We need to take into account the heat absorbed by the calorimeter itself, which has a heat capacity of 50.2 J/°C. If we assume that the temperature of the calorimeter did not change during the reaction (i.e., it remained constant), we can calculate the heat absorbed by the calorimeter:
q_calorimeter = (50.2 J/°C) * (9.3°C)
q_calorimeter = 466.86 J
The total heat produced by the reaction is then:
q_reaction = q_water + q_calorimeter
q_reaction = 3896.68 J + 466.86 J
q_reaction = 4363.54 J
Therefore, the heat produced by the reaction is 4363.54 J.
Suppose 135 g of NO3- flows into a swamp each day. What volume of N2 would be produced each day at 17.0°C and 1.00 atm if the denitrification process were complete?
____ L of N2
Suppose 135 g of NO3- flows into a swamp each day. What volume of CO2 would be produced each day at 17.0°C and 1.00 atm?
____ L of CO2
Suppose the gas mixture produced by the decomposition reaction is trapped in a container at 17.0°C; what is the density of the mixture assuming Ptotal = 1.00 atm?
____ g/L
The volume of N2 produced each day is approximately 24.56 L.
How to find the volume of N2First, let's find the number of moles of NO3- that flow into the swamp each day:
NO3- molar mass = 14.01 (N) + 3 * 16.00 (O) = 62.01 g/mol
135 g / 62.01 g/mol ≈ 2.177 moles of NO3-
In the denitrification process, NO3- is reduced to N2 gas. The balanced equation for denitrification is:
2NO3- → N2 + 3O2
From the stoichiometry of the reaction, we can see that 2 moles of NO3- produce 1 mole of N2. Therefore, the moles of N2 produced each day can be calculated as follows:
moles of N2 = 2.177 moles of NO3- / 2 ≈ 1.0885 moles of N2
Now we can use the ideal gas law equation to find the volume of N2 produced:
PV = nRT
where:
P = Pressure (1.00 atm)
V = Volume (in Liters)
n = Moles of N2 (1.0885 moles)
R = Ideal gas constant (0.0821 Latm/molK)
T = Temperature (17.0°C or 290.15 K)
Solving for the volume of N2:
V = nRT / P
V = (1.0885 moles) * (0.0821 Latm/molK) * (290.15 K) / (1.00 atm)
V ≈ 24.56 L
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According to the Law of Conservation of Mass, Matter cannot be created or destroyed.
Given that, if 15 grams of reactant went into the reaction, then how many grams of products are formed?
NH,NO,
N₂ +
H₂O
Answer:
Explanation:
According to the Law of Conservation of Mass, matter cannot be created or destroyed in a chemical reaction. Therefore, the mass of the reactants must be equal to the mass of the products.
If 15 grams of reactant went into the reaction, then the mass of the products formed must also be 15 grams. This assumes that the reaction is complete and no reactants are left unreacted.
It is important to note that this applies to closed systems where there is no loss or gain of mass. In real-world situations, some mass may be lost due to factors such as evaporation or incomplete reactions, which can affect the accuracy of the calculations.
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2. Using the law of conservation of mass, explain why the following reaction is
wrong: HCI + NaOH → NaCl.
According to the law of conservation of mass, the mass of the reactant must be equal to the mass of the product, hence the reaction is wrong
What is the conservation of mass?The law of conservation of mass states that mass within a closed system remains the same over time.
It states that the mass in an isolated system can neither be created nor be destroyed but can be transformed from one form to another.
Thus, the mass of the reactants must be equal to the mass of the products for a low energy thermodynamic process.
From the information given, we have the reaction written as;
HCI + NaOH → NaCl
The mass of the reactant Hydrogen(H) is not found on the product
The mass of the reactant(Oxygen) is also not found
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Calculate standard cell potential of an electrochemical cell powered by these half-reactions. (Write values to two decimal places. If a value is less than 1, be sure to write a 0 before the decimal.)
Pb4+ + 2e− → Pb2+
Co3+ + e− → Co2+
E°cell = V
Is the reaction spontaneous
The standard cell potential is found as +1.95 V and is a spontaneous reaction.
What is standard cell potential ?The standard cell potential (E°cell) of an electrochemical cell is given by the difference between the standard reduction potentials of the two half-cells involved.
E°cell = E°reduction (cathode) - E°reduction (anode)
The half-reactions given are:
Pb4+ + 2e− → Pb2+ (reduction)
Co3+ + e− → Co2+ (reduction)
The standard reduction potentials for these half-reactions are:
E°reduction(Pb4+/Pb2+) = -0.13 V
E°reduction(Co3+/Co2+) = +1.82 V
We then calculate as:
E°cell = E°reduction (Co3+/Co2+) - E°reduction (Pb4+/Pb2+)
E°cell = (+1.82 V) - (-0.13 V)
E°cell = +1.95 V
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What is the S-P difference (sec)?
What is the amplitude (mm)?
What isthe distance (km)?
What is the magnitude (M)?
The S-P difference (sec) is the time gap between the arrival of the S-wave and the arrival of the P-wave at a seismic station. The S-P discrepancy is depicted in the figure as 20 seconds.
The amplitude (mm) of a seismic wave is the largest displacement from its resting point. The amplitude of the waves is not depicted in the image and cannot be calculated based on the information provided.
Distance (km): Using the S-P time difference and the known velocity of seismic waves, the distance from the seismic station to the earthquake epicenter may be determined. Seismic wave velocity is determined by the type of wave and the features of the Earth's interior. The velocity of P-waves in the Earth's crust, for example, is around 6 km/s. We may compute the distance to the epicenter using this value and the S-P difference of 20 seconds as follows:
Distance = Speed x Time = 6 km/h x 20 seconds = 120 kilometres
As a result, the distance between the seismic station and the earthquake epicenter is about 120 km.
The magnitude of an earthquake (M) is a measurement of the energy generated by the earthquake based on the amplitude of the seismic waves and the distance to the epicenter. Magnitude is commonly measured on a logarithmic scale, with each whole number reflecting a factor of ten increase in energy release.
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How many grams of zinc would you need to produce 8.45 grams of hydrogen?
Zn + H2SO4 --> ZnSO4 + H2
273.8 grams of zinc (Zn) are needed to produce 8.45 grams of hydrogen gas [tex](H_2).[/tex]
In this chemical reaction, zinc (Zn) reacts with sulfuric acid [tex](H_2SO_4)[/tex] to produce zinc sulfate [tex](ZnSO_4)[/tex] and hydrogen gas [tex](H_2).[/tex]
From the balanced chemical equation, we can see that 1 mole of zinc (Zn) reacts with 1 mole of sulfuric acid [tex](H_2SO_4)[/tex] to produce 1 mole of hydrogen gas [tex](H_2).[/tex]
Hydrogen gas has a molar mass of 2.016 g/mol.
Therefore, 8.45 grams of hydrogen gas is equal to 8.45 g / 2.016 g/mol = 4.19 moles of [tex]H_2[/tex].
Since 1 mole of Zn reacts with 1 mole of [tex]H_2[/tex] , we need 4.19 moles of Zn to produce 4.19 moles of [tex]H_2[/tex].
molar mass of Zinc = 65.38 g/mol.
Therefore, 4.19 moles of Zn has a mass of 4.19 moles x 65.38 g/mol = 273.8 grams.
Therefore, you would need 273.8 grams of zinc (Zn) to produce 8.45 grams of hydrogen gas [tex](H_2).[/tex]
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please help me with this lab i wasn’t here for!
3. now that you have the mass of the NaHCO3 reactant, and the mass of the product NaCI , convert each to moles and compare to the mole ratio from your balanced equation C space below for your calculations
mass NaHCO3:
mass NaCI:
moles NaHCO3:
moles NaCI:
does the mole to mole ratio for your reaction? Agree with the ratio for the balanced equation?___
4. which reactant is the excess reactant for your reaction, how do you know?
5. Using the limiting reactant calculate the maximum amount of product that can be made from this reaction.
6. using the theoretical yield in the mass of the product that you put produce calculate percent yield.
calculations:
question #3: converting mass to moles
question #5: calculating the theoretical yield
question #6: calculating percent yield
Question #3: 0.8 g of NaHCO3 mass NaCI weight: 0.4 g 0.8 g/84 g/mol, or 0.0095 moles, of NaHCO3 0.4 g/58.5 g/mol = 0.0068 moles of NaCI are the moles.
The reaction's mole to mole ratio and the ratio in the balanced equation (1:1) are in agreement. The highest quantity of NaCI that may be produced from this reaction is 0.0095 moles since NaHCO3 is the limiting reactant.
The theoretical yield of NaCI is 0.0095 moles, which is question #6. The finished product weighs 0.4 g. The percent yield is 0.4 g/0.0095 moles times 100, which is 42.1%.
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50cm³ of 1.0M hydrochloric acid reacted with excess zinc. i) Write the equation for the reaction. ii) How many mole of aqueous hydrogen ions were present in the acid solution? iii) Calculate the volume of gas evolved at s.t.p. [Molar volume = 22.4 dm³ at s.t.p. of gas].
i) The equation for the reaction between hydrochloric acid and zinc is:
[tex]Zn + 2HCl → ZnCl2 + H2[/tex]
ii) n(HCl) = C × V = 1.0M × 0.05 L = 0.05 moles
iii) The volume of gas evolved at STP is 0.544 L or 544 mL.
The concentration of hydrochloric acid is 1.0M, which means that there is 1 mole of hydrochloric acid in 1 liter (1000 cm³) of solution. The volume of the hydrochloric acid used is 50 cm³, which is 0.05 liters.
According to the stoichiometry of the reaction, each mole of hydrochloric acid produces one mole of hydrogen ions, so the number of moles of hydrogen ions in the solution is also 0.05 moles.
The volume of gas evolved can be calculated from the ideal gas law:
PV = nRT
where P is the pressure of the gas, V is the volume of the gas, n is the number of moles of the gas, R is the gas constant (0.0821 L·atm/K·mol), and T is the temperature of the gas in Kelvin. At standard temperature and pressure (STP), the pressure is 1 atm and the temperature is 273 K. The molar volume of a gas at STP is 22.4 L/mol.
From the equation for the reaction, we know that one mole of hydrogen gas is produced for every two moles of hydrochloric acid used. Therefore, the number of moles of hydrogen gas produced is:
n(H2) = 0.5 × n(HCl) = 0.5 × 0.05 moles = 0.025 moles
Using the ideal gas law, we can calculate the volume of hydrogen gas produced at STP:
V(H2) = n(H2) × RT/P = 0.025 mol × 0.0821 L·atm/K·mol × 273 K/1 atm = 0.544 L
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5 moles of a monoatomic ideal gas is compressed reversibly and adiabatically. The initial volume is 6 dm3 and the final volume is 2 dm3. The initial temperature is 27°C.
(i) What would be the final temperature in this process?
(ii) Calculate w, q and ΔE for the process. Given Cv = 20.91 J K−1 mol−1, γ = 1.4
Final temperature: 677.4K. Work done: -7026J.
Heat exchanged: 0J. Change in internal energy: -7026J.
How to solve(i) For an adiabatic process, T1(V1)^γ-1 = T2(V2)^γ-1.
When we substitute the values (γ=1.4, T1=300K, V1=6dm³, V2=2dm³), we get T2 = 677.4K.
(ii) w = -(P1V1 - P2V2)/(γ-1) = -(nRT1 - nRT2)/(γ-1) = -5 * 8.314 * (677.4 - 300) / 0.4 = -7026J.
For adiabatic, q = 0. ΔE = q + w = -7026J (since q=0).
Final temperature: 677.4K. Work done: -7026J.
Heat exchanged: 0J. Change in internal energy: -7026J.
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Pleae answer 2a and 2b
A chemical interaction between an acid and a base is known as an acid-base reaction.
Thus, These are known as acid-base theories, such as the Brnsted-Lowry acid-base theory, and they offer alternative conceptions of the reaction mechanisms and their application in solving related problems.
When examining acid-base reactions for gaseous or liquid species, or when the acid or basic character may be less obvious, their significance becomes clear.
The relative potency of the conjugated acid-base pair in the salt controls the pH of its solutions when weak acids and bases react. The resulting salt or its solution can be basic, neutral, or acidic. A strong acid and a weak base can combine to generate an acid salt.
Thus, A chemical interaction between an acid and a base is known as an acid-base reaction.
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4. A silver bar with a mass of 300 grams is heated from 30 °C to 55 °C. How much heat does the silver ber absorb in joules? In kilojoules? The specific heat of silver is 0.235 g C
A silver bar with the mass of the 300 grams is heated from the 30 °C to 55 °C. The amount heat does the silver bar absorb in the joules is 1762.5 J.
The mass of the silver bar = 300 g
The initial temperature = 30 °C
The final temperature = 55 °C
The heat energy is expressed as :
Q = mc ΔT
Where,
The m is mass of the silver bar = 300 g
The c is the specific heat capacity = 0.235 J/g °C
The ΔT is the change in the temperature = final temperature - initial temperature
The ΔT is the change in the temperature = 55 °C - 30 °C
The ΔT is the change in the temperature = 25 °C
The heat energy, Q = 300 × 0.235 × 25
The heat energy, Q = 1762.5 J
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How many g Al must react with iodine to form AlI₃ via the following reaction scheme to release -836.0 kJ of heat? 2 Al(s) + 3 I₂(s) → 2 AlI₃(s)
∆H = -302.9 kJ
The mass (in grams) of aluminum, Al that must react with iodine to form AlI₃, given that -836.0 KJ of heat is relaesd is 149.0 g
How do i determine the mass aluminum required?The mass of aluminum required to react with iodine to produce AlI₃ can be obtain as shown below:
2Al(s) + 3I₂(s) → 2AlI₃(s) ∆H = -302.9 KJ
Molar mass of aluminum, Al = 27 g/molMass of aluminum, Al from the balanced equation = 2 × 27 = 54 gFrom the balanced equation above,
When -302.9 KJ of heat energy is released, 54 g of aluminum, Al reacted.
Therefore,
When -836.0 KJ of heat energy will be release = (-836.0KJ × 54 g) / -302.9 KJ = 149.0 g of aluminum, Al will react.
Thus, from the above calculation, we can conclude that the mass of aluminum, Al required is 149.0 g
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What was the effect of the addition of FeCl3 to the sample solution in the dichromate titration? Explain
[tex]FeCl_3[/tex] is added to ensure all reducing agent is oxidized, indicating endpoint in dichromate titration.
In a dichromate titration, [tex]FeCl_3[/tex] is frequently added to the example arrangement as a sign of the endpoint. The expansion of [tex]FeCl_3[/tex] to the example arrangement assists with guaranteeing that the lessening specialist has been all oxidized by the potassium dichromate ([tex]K_2Cr_2O_7[/tex] ) arrangement.
[tex]FeCl_3[/tex] responds with any overabundance[tex]K_2Cr_2O_7[/tex] in the answer for structure a red-earthy colored encourage of[tex]Fe(OH)_3[/tex] , demonstrating that the lessening specialist has been all oxidized. This response is known as a "back-titration" since overabundance[tex]K_2Cr_2O_7[/tex] is added to the arrangement, trailed by the option of [tex]FeCl_3[/tex] to decide how much unreacted [tex]K_2Cr_2O_7[/tex] .
The response somewhere in the range of [tex]FeCl_3[/tex] and [tex]K_2Cr_2O_7[/tex] can be addressed as:
[tex]6FeCl_3 + K_2Cr_2O_7 + 7H_2SO_4 → 3Fe_2(SO_4)_3 + Cr_2(SO_4)_3 + K_2SO_4 + 7H_2O + 3Cl_2[/tex]
The [tex]FeCl_3[/tex] goes about as a pointer in this response since it responds with the overabundance [tex]K_2Cr_2O_7[/tex] until the decreasing specialist has been all oxidized. As of now, the red-earthy colored encourage of [tex]Fe(OH)_3[/tex] structures, showing that the endpoint has been reached.
Without the expansion of [tex]FeCl_3[/tex], it would be challenging to precisely decide the endpoint of the titration. The expansion of [tex]FeCl_3[/tex] is important to guarantee that the lessening specialist has been all oxidized and that the endpoint has been reached, considering a more exact assurance of the grouping of the diminishing specialist in the example arrangement.
In outline, the expansion of [tex]FeCl_3[/tex] to the example arrangement in a dichromate titration is significant in light of the fact that it assists with guaranteeing that the decreasing specialist has been all oxidized, considering a more precise assurance of its focus.
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The complete question is -
What is the reason for a dichromate titration, and how does [tex]FeCl_3[/tex]support deciding the endpoint of the titration? Might you at any point give the compound condition to the response somewhere in the range of [tex]FeCl_3[/tex] and [tex]K_2Cr_2O_7[/tex] and make sense of why [tex]FeCl_3[/tex] goes about as a marker in this response?
what is the ph of a .100M naclo solution
The pH of a 0.100M NaClO solution is 1.
How to calculate pH?pH, meaning power of hydrogen, is a measure of how acidic/basic a solution is. The range goes from 0 - 14, with 7 being neutral. pHs of less than 7 indicate acidity, whereas a pH of greater than 7 indicates a base.
pH is really a measure of the relative amount of free hydrogen and hydroxyl ions in the water. It can be estimated using the following formula;
pH = - log {H+}
Where;
H+ = hydrogen ion concentrationpH = - log {0.100}
pH = 1
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If the initial temperature of an ideal gas at 2.250 atm
is 62.00 ∘C,
what final temperature would cause the pressure to be reduced to 1.700 atm?
Review-Chemical Reactions
Write balanced chemical equations for the following reactions:
a. chlorine gas and aqueous sodium iodide react to form aqueous sodium chloride and
solid iodine
b. solid sodium chlorate is heated to form solid sodium chloride and oxygen gas
c. solid potassium reacts with liquid water to produce aqueous potassium hydroxide and
hydrogen gas
Answer:
a. Cl2 (g) + 2NaI (aq) → 2NaCl (aq) + I2 (s)
b. 2NaClO3 (s) → 2NaCl (s) + 3O2 (g)
c. 2K (s) + 2H2O (l) → 2KOH (aq) + H2 (g)
Explanation:
determine the solubility of NH and 90° C
The solubility of NH₃ in water at 90°C is approximately 0.03 g per 100 g of water.
What is the solubility of NH₃?The solubility can be determined from a solubility table or by using the appropriate equilibrium constant.
According to a solubility table, the solubility of ammonia in water at 90°C is approximately 88 g per 100 g of water.
Alternatively, the equilibrium constant for the dissolution of ammonia in water at 90°C can be used to calculate the solubility.
The equilibrium constant (K) for the reaction:
NH3 (g) + H2O (l) ⇌ NH4+ (aq) + OH- (aq)
is approximately 1.76 x 10⁻⁵ at 90°C.
Using the equilibrium constant expression:
K = [NH4+][OH-]/[NH3][H2O]
Assuming that the concentration of water remains constant at 100 g per 100 g of solution, and that the concentration of NH4+ and OH- are negligible compared to that of NH3, the solubility of NH3 can be calculated as:
[NH3] = K[H2O] = 1.76 x 10⁻⁵ x 100 = 1.76 x 10⁻³ mol/L
Converting to grams per 100 g of water:
1.76 x 10⁻³ mol/L x 17.03 g/mol = 0.03 g/100 g of water
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The complete question is below:
determine the solubility of NH₃ in water at 90° C
Can someone explain the Glyceraldehyde structure for me in detail please. I read that the first carbon atom is the only asymmetric one out of all three carbons and that the other two carbons do have four attachments that just aren’t different. I can’t even see how the atoms have four attachments though.
Answer:
Glyceraldehyde is a simple sugar with three carbon atoms attached to hydroxyl and hydrogen or carbonyl groups. The first carbon atom has four different groups, including an aldehyde group, which makes it asymmetric. This results in two stereoisomers, D-glyceraldehyde and L-glyceraldehyde, that are mirror images of each other and have opposite optical activities.
Which of these are part of the
Earth's lithosphere?
O clouds
O glaciers
O mountains
O water vapor
Compared to chemical reactions, most nuclear reactions result in the
OA. formation of new compounds
OB. formation of new elements
O C. formation of new bonds
OD. loss of valence electrons
Answer:
OB. formation of new elements.
Nuclear reactions involve changes in the nucleus of an atom, such as the splitting of a nucleus or the combining of two nuclei. These reactions can result in the formation of new elements, as the number of protons in the nucleus determines the element. In contrast, chemical reactions involve the rearrangement of electrons between atoms to form new compounds, but do not involve changes to the nucleus.
Predict which of the following reactions has a positive change in entropy.
I. 2N2(g) + O2(g) → 2N2O(g)
II. CaCO3(s) → CaO(s) + CO2(g)
III. Zn(s) + 2HCl(aq) → ZnCl2(aq) + H2(g)
Answer:
Explanation:
The change in entropy of a system can be determined by comparing the entropy of the reactants to the entropy of the products. The reaction that leads to an increase in the number of moles of gas or particles will generally have a positive change in entropy.
I. 2N2(g) + O2(g) → 2N2O(g)
The reactants have 3 moles of gas, while the product also has 3 moles of gas. Therefore, there is no change in the number of moles of gas, and the change in entropy is likely to be small.
II. CaCO3(s) → CaO(s) + CO2(g)
The reactant is a solid, while the products are a solid and a gas. The formation of a gas from a solid leads to an increase in the number of moles of particles, and therefore an increase in entropy.
III. Zn(s) + 2HCl(aq) → ZnCl2(aq) + H2(g)
The reactants consist of a solid and a liquid, while the products consist of an aqueous solution and a gas. The formation of a gas leads to an increase in the number of moles of particles, and therefore an increase in entropy.
Therefore, reactions II and III have a positive change in entropyentropy
I2 + N2H4==> HI + N2 according to the reaction ,How many grams of HI are obtained if 115.7 g of N2H4 reacts with
an excess of iodine?
The mass of the HI that is produced is 1843 g
What is stoichiometry?Stoichiometry is a branch of chemistry that focuses on the quantitative relationships in chemical reactions between reactants and products.
What is the number of moles?
Number of moles of [tex]N_{2} H_{4}[/tex] = 115.7 g/32 g/mol
= 3.6 moles
Now we have that the balanced reaction equation is;
[tex]N_{2} H_{4} + 2I_{2} --- > N_{2} + 4 HI[/tex]
If 1 mole of [tex]N_{2} H_{4}[/tex] produces 4 moles of HI
3.6 moles of [tex]N_{2} H_{4}[/tex] will produce 3.6 * 4/1
= 14.4 moles of HI
Mass of HI produced = 14.4 moles * 128 g/mol
= 1843 g
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A student has a 2.97 L
bottle that contains a mixture of O2
, N2
, and CO2
with a total pressure of 5.68 bar
at 298 K
. She knows that the mixture contains 0.225 mol N2
and that the partial pressure of CO2
is 0.309 bar
. Calculate the partial pressure of O2
.
The following equations represent chemical
reactions.
Chemical Reactions
1) 2Na+2H₂O →NaOH + H₂
2) H₂+O₂ H₂O
3) MgCl₂ → MgCl₂
4) NaOH+MgCh→ NaCl + MgOH
Which equation shows that the total mass during a chemical reaction stays the same?
The equation that shows that the total mass during a chemical reaction stays the same is 2) H₂ + O₂ → H₂O.
This is an example of a balanced chemical equation where the number of atoms of each element on both the reactant and product side is equal. In other words, the total number of atoms of each element is conserved, and therefore the total mass is conserved. In the other reactions, either the number of atoms on the product side is different from the reactant side or there is no reaction at all.
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What is the pH of the solution formed when 12.50 mL of 1.05 M KOH is added to 50.0 mL of 0.225 M HBr?
A. 0.65
B. 1.52
C. 12.48
D. 13.35
Answer: D
Explanation:
When 12.50 mL of 1.05 M KOH is added to 50.0 mL of 0.225 M HBr, the resulting solution has a pH of 13.35.
Here’s how to calculate it:
First, we need to determine the number of moles of KOH and HBr in the solution:
moles of KOH = (12.50 mL) * (1.05 mol/L) * (1 L/1000 mL) = 0.013125 mol moles of HBr = (50.0 mL) * (0.225 mol/L) * (1 L/1000 mL) = 0.01125 mol
KOH is a strong base and HBr is a strong acid, so they will react completely to form water and a salt (KBr):
KOH + HBr -> KBr + H2O
The number of moles of KOH is greater than the number of moles of HBr, so there will be an excess of KOH in the solution after the reaction is complete:
moles of excess KOH = moles of KOH - moles of HBr = 0.013125 mol - 0.01125 mol = 0.001875 mol
The total volume of the solution is the sum of the volumes of KOH and HBr:
total volume = 12.50 mL + 50.0 mL = 62.5 mL
The concentration of excess OH- ions in the solution is:
[OH-] = moles of excess KOH / total volume = 0.001875 mol / (62.5 mL * (1 L/1000 mL)) = 0.03 M
The pOH of the solution can be calculated using the formula pOH = -log[OH-]:
pOH = -log(0.03) = 1.52
The pH can be calculated using the formula pH + pOH = 14:
pH = 14 - pOH = 14 - 1.52 = 13.35
So the correct answer is D. 13.35.
The article talks mainly about A. Dr. Dituri's small underwater habitat B. Dr. Dituri's Project Neptune 100 C. Dr. Dituri's talks with other scientists D. Dr. Dituri's 28 years in the U.S. Navy
We see here that the article is actually talking about: B. Dr. Dituri's Project Neptune 100.
What is an article?A piece of writing known as an article is typically printed in a newspaper, magazine, or journal. It may address a variety of subjects, such as news, features, essays, research findings, and reviews.
We can see here that in the article, being referred to in the question is known as "A Chat With the Scientist Living Underwater for 100 Days,".
From the article, it is very clear that it refers to Dr. Dituri's Project Neptune 100. Retired Navy officer, Joseph Dituri is seeking to break the current record for longest period of time spent submerged.
Note: I can't post the article here. But I have provided the title of the article above.
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3. Litharge, Pb0, is an ore that can be roasted (heated) in the presence of carbon monoxide, CO, to produce elemental lead. The
reaction that takes place during this roasting process is represented by the balanced equation below.
PbO(s) + CO(g) → Pb(s) + CO₂(g)
In which compound does carbon have the greater oxidation number
Answer:
Explanation:
In the given reaction, carbon has a greater oxidation number in carbon dioxide (CO₂) than in carbon monoxide (CO). In CO₂, the oxidation number of carbon is +4, while in CO it is +2.
Question 8 of 21
Which nucleus completes the following equation?
The nucleus completing the following equation is option C: ₂₄⁵⁰Cr.
This reaction is a type of radioactive nuclei decay.
What is radioactive decay?Radioactive decay is the process by which unstable atomic nuclei undergo spontaneous transformations in order to achieve a more stable state. This is accomplished by the emission of particles and/or electromagnetic radiation from the nucleus. The decay may occur by several mechanisms, including alpha decay, beta decay, gamma decay, and electron capture.
In alpha decay, the nucleus emits an alpha particle, which consists of two protons and two neutrons, resulting in a daughter nucleus that has two fewer protons and two fewer neutrons than the original nucleus.
In beta decay, a neutron in the nucleus is converted into a proton and an electron, and the electron is then emitted from the nucleus as a beta particle. This results in the daughter nucleus having one more proton and one fewer neutron than the original nucleus.
In gamma decay, the nucleus emits a gamma ray, which is a high-energy electromagnetic radiation, without changing the number of protons or neutrons in the nucleus.
In electron capture, an electron from the inner shell of the atom is captured by the nucleus, and a proton in the nucleus is converted into a neutron. This results in the daughter nucleus having one fewer proton and one more neutron than the original nucleus.
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