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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A 192 gram piece of copper was heated to 100.°C in a boiling water bath, then it was dropped into a beaker containing 850. mL of water at 4.00°C. What is the final temperature of the copper and water after they come to thermal equilibrium?
Note: The specific heat of copper is 0.385 J/g °C.
Do not round your answer in the middle of the problem. Round at the very end.
Round your answer to the correct number of sig figs. Your units should be degrees Celsius.
The final temperature of the copper and water after they come to thermal equilibrium is 109.8°C.
What is temperature?Temperature is a measure of the amount of thermal energy present in a substance or object. It is measured in degrees on a scale such as Fahrenheit, Celsius, or Kelvin. Temperature is important in determining the physical and chemical properties of a substance, such as its melting point, boiling point, and specific gravity. Temperature also affects the rate of a chemical reaction and the speed of diffusion.
The change in temperature of the copper can be calculated using the equation
ΔT = (Q/mc), where Q is the heat transferred, m is the mass of the copper, and c is the specific heat of copper.
Q = mcΔT = (192 g)(0.385 J/g °C)(100°C) = 74080 J
The heat transferred from the copper must equal the heat transferred to the water. Therefore,
(74080 J) = (0.85 L)(4.184 J/g°C)(ΔT)
ΔT = (74080 J)/[(0.85 L)(4.184 J/g°C)] = 109.8°C
The final temperature of the copper and water after they come to thermal equilibrium is 109.8°C.
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Calculate the energy difference (deltaE, in Joules) of an electron's transition from n = 6 to n = 1 in a hydrogen atom.
The energy difference of an electron's transition from n = 6 to n = 1 in a hydrogen atom is approximately -2.17 × 10⁻¹⁸ Joules.
To calculate the energy difference (deltaE) of an electron's transition from n = 6 to n = 1 in a hydrogen atom, we can use the following equation:
deltaE = -13.6 * (1/n_final^2 - 1/n_initial^2) eV
where n_initial is the initial energy level (6 in this case), n_final is the final energy level (1 in this case), and -13.6 eV is the ionization energy of hydrogen.
Converting eV to Joules, we get:
1 eV = 1.602 x 10^-19 J
Therefore, deltaE in Joules can be calculated as follows:
deltaE = -13.6 * (1/1^2 - 1/6^2) * 1.602 x 10^-19 J/eV
deltaE = -2.179 x 10^-18 J
Therefore, the energy difference (deltaE) of an electron's transition from n = 6 to n = 1 in a hydrogen atom is -2.179 x 10^-18 J.
To calculate the energy difference (ΔE) for an electron's transition from n = 6 to n = 1 in a hydrogen atom, you can use the following formula:
ΔE = -13.6 eV * (1/nf² - 1/ni²)
Where ΔE is the energy difference in electron volts (eV), nf is the final energy level (1 in this case), and ni is the initial energy level (6 in this case).
ΔE = -13.6 eV * (1/1² - 1/6²)
ΔE ≈ -13.56 eV
Now convert electron volts to Joules:
1 eV = 1.6 × 10⁻¹⁹ J
ΔE ≈ -13.56 eV * 1.6 × 10⁻¹⁹ J/eV
ΔE ≈ -2.17 × 10⁻¹⁸ J
So, approximately -2.17 × 10⁻¹⁸ Joules is the energy difference of an electron's transition from n = 6 to n = 1 in a hydrogen atom.
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Lead(II) nitrate and ammonium iodide react to form lead(II) iodide and ammonium nitrate according to the reaction
Pb(NO3)2(aq)+2NH4I(aq)⟶PbI2(s)+2NH4NO3(aq)
What volume of a 0.350 M NH4I solution is required to react with 415 mL of a 0.120 M Pb(NO3)2 solution?
How many moles of PbI2 are formed from this reaction?
1. The volume of 0.350 M NH₄I solution is required is 286 mL
2. The mole of PbI₂ formed is 0.0498
1. How do i determine the volume of NH4I required?First, we shall determine the mole in 415 mL of 0.120 M Pb(NO₃)₂. Details below:
Molarity of Pb(NO₃)₂ = 0.120 M MVolume of Pb(NO₃)₂ = 415 mL = 415 / 1000 = 0.415 LMole of Pb(NO₃)₂ =?Mole = molarity × volume
Mole of Pb(NO₃)₂ = 0.120 × 0.415
Mole of Pb(NO₃)₂ = 0.0498 mole
Next, we shall determine the mole of NH₄I that reacted. Details below:
Pb(NO₃)₂(aq) + 2NH₄I(aq) ⟶ PbI₂(s) + 2NH₄NO₃(aq)
From the balanced equation above,
1 moles of Pb(NO₃)₂ reacted with 2 moles of NH₄I
Therefore,
0.0498 mole of Pb(NO₃)₂ will react with = 0.0498 × 2 = 0.1 mole of NH₄I
Finally, we shall determine the volume of NH₄I required for the reaction. Details below:
Molarity of NH₄I = 0.350 MMole of NH₄I = 0.1 moleVolume of NH₄I =?Volume = mole / molarity
Volume of NH₄I = 0.1 / 0.350
Volume of NH₄I = 0.286 L
Multiply by 1000 to express in mL
Volume of NH₄I = 0.286 × 1000
Volume of NH₄I = 286 mL
2. How do i determine the mole of PbI₂ formed?The mole of PbI₂ formed can be obtain as follow:
Pb(NO₃)₂(aq) + 2NH₄I(aq) ⟶ PbI₂(s) + 2NH₄NO₃(aq)
From the balanced equation above,
1 mole of Pb(NO₃)₂ reacted to produced 1 mole of PbI₂
Therefore,
0.0498 mole of Pb(NO₃)₂ will also react to produce 0.0498 mole of PbI₂
Thus, the number of mole of PbI₂ formed is 0.0498 mole
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What volume of oxygen gas can be collected
at 1.05 atm pressure and 44.0◦C when 42.5 g
of KClO3 decompose by heating, according to
the following equation?
2 KClO3(s) ∆
−−−−→
MnO2
2 KCl(s) + 3 O2(g)
Answer in units of L.
005 1.0 points
The volume of oxygen gas, O₂ collected at 1.05 atm pressure and 44.0 °C when 42.5 g of KClO₃ decomposed is 13.01 L
How do i determine the volume of oxygen gas collected?We shall begin by obtaining the mole in 42.5 g of KClO₃. Details below:
Mass of KClO₃ = 42.5 g Molar mass of KClO₃ = 122.5 g/mol Mole of KClO₃ =?Mole = mass / molar mass
Mole of CaC₂ = 42.5 / 122.5
Mole of CaC₂ = 0.35 mole
Next, we shall determine the mole of oxygen gas, O₂. produced. Details below:
2KClO₃ -> 2KCl + 3O₂
From the balanced equation above,
2 moles of KClO₃ decomposed to produced 3 mole of O₂
Therefore,
0.35 mole of KClO₃ will decompose to produce = (0.35 × 3) / 2 = 0.525 mole O₂
Finally, we shall determine the volume of oxygen gas, O₂ collected. Details below:
Pressure (P) = 1.05 atmTemperature (T) = 44 °C = 44 + 273 = 317 KGas constant (R) = 0.0821 atm.L/mol KNumber of mole (n) = 0.525 moleVolume of gas (V) =?PV = nRT
1.05 × V = 0.525 × 0.0821 × 317
Divide both sides by 1.05
V = (0.525 × 0.0821 × 317) / 1.05
Volume of oxygen gas = 13.01 L
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How does the presence of coal in Antarctica support Wegener's continental drift hypothesis?
Answer:
Explanation:
Coal deposits have been found in Antarctica, particularly in the Transantarctic Mountains where they are interbedded in sedimentary rocks of the flat-lying Beacon Supergroup. The presence of coal in Antarctica supports Wegener's continental drift hypothesis because it suggests that Antarctica was once part of a larger landmass that had a warm climate suitable for the formation of coal. Coal is formed from ancient plant matter that has been compressed and heated over millions of years. The presence of coal in Antarctica suggests that the continent was once located closer to the equator and had a climate that supported lush vegetation.
2. A slice of chocolate cake contains 560 Calories. a. Determine the number of calories found in the slice of cake. b. Determine the number of joules of energy for the slice of cake. c. Determine the number of kilojoules of energy for the slice of cake. 3. Determine the number of calories in 1.5 kilojoules of energy.
SHIW WORK
b. To determine the number of joules of energy for the slice of cake, we need to convert the calories to joules using the conversion factor 1 calorie = 4.184 joules:
Number of joules = 560 calories * 4.184 joules/calorie = 2343.04 joules
Therefore, the slice of cake contains 2343.04 joules of energy.
c. To determine the number of kilojoules of energy for the slice of cake, we can divide the number of joules by 1000:
Number of kilojoules = 2343.04 joules / 1000 = 2.34304 kilojoules
Therefore, the slice of cake contains 2.34304 kilojoules of energy.
To determine the number of calories in 1.5 kilojoules of energy, we need to convert kilojoules to calories using the conversion factor 1 kilojoule = 1000 calories:
Number of calories = 1.5 kilojoules * 1000 calories/kilojoule = 1500 calories
Therefore, 1.5 kilojoules of energy contains 1500 calories.
Explanation:
Answer:
2. a. 560 Calories, b. 2343.04 J, c. 2.34304 kJ
3. 358.508604 Cal
Explanation:
2.
a. The number of calories found in the slice of chocolate cake is 56012.
b. To determine the number of joules of energy for the slice of cake, we can use the conversion factor that 1 calorie is equal to 4.184 joules3. Therefore, the number of joules in the slice of cake is:
560 Cal ⋅ 4.184 J/ 1 Cal = 2343.04J
c. To determine the number of kilojoules of energy for the slice of cake, we can use the conversion factor that 1 kilojoule is equal to 1000 joules4. Therefore, the number of kilojoules in the slice of cake is:
2343.04 J ⋅ 1 kJ/1000 J = 2.34304 kJ
3. To determine the number of calories in 1.5 kilojoules of energy, we can use the conversion factor that 1 kilojoule is equal to 239.005736 calories1. Therefore, the number of calories in 1.5 kilojoules of energy is:
1.5 kJ ⋅ 239.005736 Cal / 1 kJ = 358.508604 Cal
( + 0₂ (0₂ 1 Is the molecular mas of carbon is 12 and that of oxygen is 32, Calculate the mass of carbon dioxide formed when 24kg of carbon is burnt completely in oxygen and determine the heat thereby released in MJ if the complete combustion of 1kg of carbon releases 33.8MJ of heat
The mass of carbon dioxide formed when 24 kg of carbon is burnt completely in oxygen is 88 kg, and the heat released is 811.2 MJ.
What is Molar Mass?
Molar mass is the mass of one mole of a substance and is expressed in grams per mole (g/mol). It is calculated by adding up the atomic masses of all the atoms in a molecule or formula unit of a compound. The molar mass is used in stoichiometry calculations to convert between mass and moles of a substance.
The balanced equation for the combustion of carbon is:
C + O₂ → CO₂
From the equation, we can see that one mole of carbon reacts with one mole of oxygen to produce one mole of carbon dioxide. The molar mass of carbon dioxide is 12 + (2 × 16) = 44 g/mol.
First, let's find the number of moles of carbon in 24 kg:
n(C) = m/M = 24000 g / 12 g/mol = 2000 mol
Therefore, 2000 mol of CO₂ will be produced.
The mass of CO₂ produced can be calculated as:
m(CO₂) = n(CO₂) × M(CO₂) = 2000 mol × 44 g/mol = 88,000 g = 88 kg
Now, let's calculate the heat released during combustion:
Heat released = 33.8 MJ/kg × 24 kg = 811.2 MJ
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A 2.550×10−2 M glycerol solution (C3H8O3) in water is at 20.0 ∘C . The sample was created by dissolving a sample of C3H8O3 in water and then bringing the volume up to 1.000 L. It was determined that the volume of water needed to do this was 998.9 mL. The density of water at 20.0 ∘C is 0.9982 g/mL
a.) Calculate the molality of the glycerol solution
b.) Calculate the mole fraction of glycerol in this solution
c.) Calculate the concentration of the glycerol solution in percent by mass
d.) Calculate the concentration of the glycerol solution in parts per million by mass
The molality of the solution is 0.0256 m.
The mole fraction of glycerol is 0.00046
The percent by mass concentration of glycerol is 0.23%
The ppm concentration is 2300 ppm
What is the molality?Molality is a measure of the concentration of a solute in a solution. It is defined as the number of moles of solute per kilogram of solvent.
The formula for molality is:
molality = moles of solute / mass of solvent in kilograms
1) Density of water = mass/volume
Mass of water = Density * volume of water
Mass =[tex]0.9982 g/mL * 998.9 mL[/tex]
Mass =0.997 Kg of water
Number of moles of the glycerol = [tex]2.550* 10^-2 M * 1 L[/tex]
= [tex]2.550*10^-2[/tex] moles
Molality of the solution = [tex]2.550*10^-2[/tex] moles/0.997 Kg
= 0.0256 m
Number of moles of water = 998.9/18 g/mol
= 55.5 mole
Mole fraction of glycerol = [tex]2.550*10^-2[/tex] /[tex]2.550*10^-2[/tex] + 55.5
= 0.00046
By percent by mass;
2.3/1001.2 * 100/1
= 0.23%
Mass of glycerol = 2.3 g
Volume of solution = 1 L
Thus we have concentration in ppm as;
[tex]2.3 * 10^3[/tex] mg/ 1 L =2300 ppm
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Haw many valance electrons in the following atoms.
O Na Sr
Answer:O has 6, Na has 1, and Sr has 2.
Explanation:
What amount of heat, in kJ, is required to vaporize 181.20 g of ethanol (C₂H₅OH)? (∆Hvap = 43.3 kJ/mol)
The amount of heat required to vaporize 181.20 g of ethanol would be 170.1 kJ.
Heat of vaporizationUsing the formula:
Q = n ∆Hvap
where:
Q is the amount of heat required to vaporizen is the number of moles of the substance∆Hvap is the molar heat of vaporization.Moles of 181.20 g of ethanol = 181.20 g / 46.07 g/mol = 3.933 mol
Substituting the values:
Q = 3.933 mol x 43.3 kJ/mol = 170.1 kJ
In other words, the amount of heat required to vaporize 181.20 g of ethanol is 170.1 kJ.
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Three of the primary components of air are
carbon dioxide, nitrogen, and oxygen. In a
sample containing a mixture of only these
gases at exactly one-atmosphere pressure, the partial pressures of carbon dioxide and nitrogen are given as PCO2 = 0.285 torr and
PN2 = 580.502 torr. What is the partial pressure of oxygen?
Answer in units of torr.
The partial pressure of the oxygen is 0.236 atm.
What is partial pressure?The pressure that one gas component in a mixture of gases exerts is known as partial pressure. It is the pressure that the gas would experience if it took up the same amount of space in the mixture at the same temperature on its own.
We know that;
P[tex]CO_{2}[/tex] = 0.285 torr or 0.000375 atm
P[tex]N_{2}[/tex] = 580.502 torr or 0.764 atm
P[tex]O_{2}[/tex] = ?
Total pressure = 1 atm
Then we have that;
PT =P[tex]CO_{2}[/tex] +P[tex]N_{2}[/tex]+ P[tex]O_{2}[/tex]
P[tex]O_{2}[/tex] = PT - (P[tex]CO_{2}[/tex] + P[tex]N_{2}[/tex])
P[tex]O_{2}[/tex] = 1 - (0.000375 + 0.764)
P[tex]O_{2}[/tex]= 0.236 atm
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What is the net ionic charge of an oxygen ion ?
2ch4 and c2h8 how are they different
Answer:
Explanation:
Both 2CH4 and C2H8 have the same number and kind of elements. But practically, 2CH4 will be existing but C2H8 cannot exist.
100 POINTS PLEASE HELP!!! 1. Explain how you would determine the enthalpy of reaction for the hypothetical reaction A2X4(l) + X2(g) → 2AX3(g) using the following information. You do not need to calculate an answer. Respond to the prompt with a minimum response length of 50 words.
To determine the enthalpy of reaction for the given reaction, use Hess's Law, which states that the total enthalpy change of a reaction is independent of the pathway between the initial and final states.
How to determine the enthalpy of reaction?Break the given reaction into a series of steps for which the enthalpy changes are known or can be measured experimentally.
Add the enthalpy changes of each step to determine the overall enthalpy change for the reaction.
For example, determine the enthalpy of formation for A₂X₄(l), X₂(g), and AX₃(g) and use them to calculate the enthalpy of reaction for the given equation.
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How many moles of solute are in 2 L of an 8.0 M solution?
Answer: 4 moles i think this is right im not sure
Identity the number of bonding pairs and lone pairs of electrons n2
There are 3 bonding pairs and 7 lone pairs of electrons in N2.
What is an electronAn atom's nucleus is orbited by an electron, a subatomic particle with a negative charge. Along with protons and neutrons, it is one of the elementary particles that make up matter. The mass of an electron is exceedingly small, it is roughly 1/1836 that of a proton.
To determine the number of lone pairs of electrons in N2, we need to subtract the number of bonding pairs from the total number of valence electrons:
Number of lone pairs = Total number of valence electrons - Number of bonding pairs
Number of lone pairs = 10 - 3
Number of lone pairs = 7
Therefore, there are 3 bonding pairs and 7 lone pairs of electrons in N2.
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a solution is made by mixing 100 ml of ethanol and 200 mL of water identified the solute of solvent of the solution and calculate the total volume of the solution
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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A solution of thickness 3cm transmits 30%. calculate the concentration of the solution. E= 400dm/mol/cm
The concentration of the solution is 0.000435 mol/dm³.
What is the concentration of the solution?The concentration of a solution is calculated as follows;
Concentration = (Absorbance) / (Molar absorptivity x path length)
the path length = 3cm
the molar absorptivity (E) = 400 dm/mol/cm.
if the solution transmits 30% of the light, it absorbs 70% of the incident light.
Absorbance = log (1/Transmittance)
Absorbance = log (1/0.3)
Absorbance = 0.523
Concentration = (0.523) / (400 dm/mol/cm x 3 cm)
= 0.000435 mol/dm³
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A flexible container at an initial volume of 5.12 L
contains 8.51 mol
of gas. More gas is then added to the container until it reaches a final volume of 13.3 L.
Assuming the pressure and temperature of the gas remain constant, calculate the number of moles of gas added to the container.
Step-by-step Explanation:
8.51 moles is to 5.12 L as 'x' moles is to (13.3-5.12) L
8.51 moles / 5.12 L = x / ( 13.3-5.12)
x = 13.6 moles
If the reaction A (aq) + B (aq) C(aq) has a Ka value equal to 4.26 x 10-6, what is the G value at 25 °C if the concentrations are as follows:
[A] = 1.50 M
[B] = 1.00 M
[C] = 5.00 x 10-5 M
The ΔG value for the reaction A (aq) + B (aq) → C(aq) at 25 °C and the given concentrations is -8.35 kJ/mol.
The relationship between ΔG and K is given by the following equation:
ΔG = -RTln(K)
where R is the gas constant (8.314 J/(mol·K)), T is the temperature in Kelvin (25 °C = 298.15 K), and ln denotes the natural logarithm.
To calculate K, we need to use the equilibrium expression and the given concentrations:
[tex]K = [C]/([A][B])[/tex]
[tex]K = (5.00 * 10^{-5} M)/((1.50 M)(1.00 M))[/tex]
[tex]K = 3.33 x 10^{-5}[/tex]
Now we can substitute the values for R, T, and K into the equation for ΔG:
ΔG = -RTln(K)
ΔG = [tex]-(8.314 J/(mol.K))(298.15 K)ln(3.33 x 10^{-5})[/tex]
ΔG = -8.35 kJ/mol
Therefore, the ΔG value for the reaction A (aq) + B (aq) → C(aq) at 25 °C and the given concentrations is -8.35 kJ/mol.
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Chemistry balance equation
At equilibrium, the value of K = 0.00659 for the reaction: N₂ (g) + 3 H₂ (g) ← → 2 NH₃ (g). Calculate [N₂] when [NH₃] = 0.000123 M and [H₂] = 0.0275 M
The concentration of the ammonia from the calculation is [tex]1.1 * 10^-15[/tex]M.
What is the equilibrium constant?The ratio of the concentrations of products to reactants in chemical equilibrium, for a given chemical reaction at a given temperature, is described by the equilibrium constant, abbreviated as Kc or Keq.
We can see that;
[tex]Keq = [NH_{3} ]^2/[N_{2} ] [ H_{2}]^3\\Keq[N_{2} ] [ H_{2}]^3 = [NH_{3}]^2\\\\N_{2} ] = [NH_{3}]^2/Keq[ H_{2}]^3[/tex]
=[tex](0.000123 )^2/ 0.00659 * (0.0275)^3= 1.1 * 10^-15 M[/tex]
Thus we would have the nitrogen concentration as [tex]1.1 * 10^-15[/tex] M
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A sample of an ideal gas has a volume of 2.31 L
at 279 K
and 1.01 atm.
Calculate the pressure when the volume is 1.09 L
and the temperature is 308 K.
The pressure of the gas when the volume is 1.09 L and the temperature is 308 K is 2.36 atm.
What is the final pressure of the gas?The final pressure of the gas is calculated by applying ideal gas law as follows;
(P₁V₁)/T₁ = (P₂V₂)/T₂
where
P₁, V₁, and T₁ are the initial pressure, volume, and temperature, P₂, V₂, and T₂ are the final pressure, volume, and temperature,P₂ = (P₁V₁ x T₂)/(V₂ x T₁)
P₂ = (1.01 atm x 2.31 L x 308 K) / (1.09 L x 279 K)
P₂ = 2.36 atm
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A sample of an ideal gas has a volume of 2.31 L
at 279 K
and 1.01 atm.
Calculate the pressure when the volume is 1.09 L
and the temperature is 308 K.
We can use the combined gas law to determine the pressure of the gas at the final state. 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 = 1.01 atm), volume (V1 = 2.31 L), and temperature (T1 = 279 K) of the gas, and the final volume (V2 = 1.09 L), and temperature (T2 = 308 K) of the gas. We can solve for P2, the final pressure of the gas:
(P1 x V1) / T1 = (P2 x V2) / T2
P2 = (P1 x V1 x T2) / (V2 x T1)
P2 = (1.01 atm x 2.31 L x 308 K) / (1.09 L x 279 K)
P2 = 2.41 atm (rounded to three significant figures)
Therefore, the pressure of the gas when the volume is 1.09 L and the temperature is 308 K is approximately 2.41 atm.
what is the volume and letters of a solution that contains 0.50 moles of NaOH dissolved in enough distilled water to make 3.0 mm of NaOH solution
what is the molarity of a solution that contains 60.0 G of caoh dissolved in 150 mm solution
1. To find the volume and units of a solution that contains 0.50 moles of NaOH dissolved in enough distilled water to make 3.0 M NaOH solution:
We first need to use the formula:
moles = concentration (in moles/L) x volume (in L)
Rearranging the formula to solve for volume, we get:
volume = moles / concentration
Substituting the given values, we get:
volume = 0.50 moles / 3.0 M = 0.17 L
Since the volume is given in liters, the units of the solution are L. Therefore, the solution contains 0.50 moles of NaOH dissolved in 0.17 L of distilled water, which makes a 3.0 M NaOH solution.
2. To find the molarity of a solution that contains 60.0 g of Ca(OH)2 dissolved in 150 mL of solution:
We first need to convert the mass of Ca(OH)2 to moles using the molar mass:
molar mass of Ca(OH)2 = 40.08 g/mol + 2 x 16.00 g/mol + 2 x 1.01 g/mol = 74.10 g/mol
moles of Ca(OH)2 = 60.0 g / 74.10 g/mol = 0.810 moles
Next, we need to convert the volume of the solution from milliliters to liters:
volume of solution = 150 mL / 1000 mL/L = 0.150 L
Finally, we can use the formula:
molarity = moles / volume
Substituting the given values, we get:
molarity = 0.810 moles / 0.150 L = 5.4 M
Therefore, the molarity of the solution is 5.4 M.
How many grams of zinc chloride would be formed if 77.1 grams of zinc reacts?
Zn + HCl -->ZnCl2 + H2
The amount of zinc chloride that would be formed if 77.1 grams of zinc reacts is approximately 160.77 grams
To determine how many grams of zinc chloride ([tex]ZnCl_2[/tex]) would be formed if 77.1 grams of zinc (Zn) reacts, we'll use stoichiometry.
First, we need the molar masses of the substances involved:
Zn: 65.38 g/mol
[tex]ZnCl_2[/tex] : 136.29 g/mol
Now, we'll convert grams of Zn to moles:
77.1 g Zn × (1 mol Zn / 65.38 g Zn) = 1.179 moles Zn
According to the balanced chemical equation, 1 mole of Zn reacts to form 1 mole of [tex]ZnCl_2[/tex]:
1.179 moles Zn × (1 mol ZnCl₂ / 1 mol Zn) = 1.179 moles ZnCl₂
Finally, convert moles of ZnCl₂ to grams:
1.179 moles ZnCl₂ × (136.29 g ZnCl₂ / 1 mol ZnCl₂) ≈ 160.77 g ZnCl₂
So, approximately 160.77 grams of zinc chloride would be formed if 77.1 grams of zinc reacts.
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Is the following reaction endothermic or exothermic?
C3H8 + 5 O2 --> 3 CO2 + 4 H2O
H= -2200 kJ
Since the ΔH for the given reaction has negative value, the reaction is exothermic reaction.
A reaction that is exothermic is one in which power is given off as heat or light. In contrast to an endothermic process, which draws energy from its surroundings, an exothermic reaction transfers energy into the environment. The alteration in enthalpy (H) during an exothermic reaction will be negative. Since the ΔH for the given reaction has negative value, the reaction is exothermic reaction.
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Complete combustion of a 0.0200 mol sample of a hydrocarbon, CxHy, gives 4.032 L of CO2 at STP and 3.602 g of H2O.
(a) What is the molecular formula of the hydrocarbon? (b) What is the empirical formula of the hydrocarbon?
The hydrocarbon's molecular structure is [tex]C_9H_20[/tex].The hydrocarbon's empirical formula is [tex]C_9[/tex]/4H5.
To solve this problem, we need to use stoichiometry to relate the amount of [tex]CO__2[/tex] and [tex]H_2O[/tex] produced to the amount of [tex]CxHy[/tex] burned.
(a) To find the molecular formula of the hydrocarbon, we need to first calculate the number of moles of [tex]CO__2[/tex] and [tex]H_2O[/tex] produced. From the ideal gas law, we know that 1 mole of gas at STP (standard temperature and pressure) occupies 22.4 L. Therefore, 4.032 L of [tex]CO__2[/tex] at STP corresponds to:
4.032 L / 22.4 L/mol = 0.180 mol [tex]CO__2[/tex]
Similarly, the mass of H2O produced corresponds to:
3.602 g / 18.02 g/mol = 0.200 mol [tex]H_2O[/tex]
Since the hydrocarbon undergoes complete combustion, it reacts with oxygen to form [tex]CO__2[/tex] and [tex]H_2O[/tex] according to the balanced chemical equation:
[tex]CxHy[/tex] + (x + (y/4))O2 → [tex]CO__2[/tex] + (y/2)[tex]H_2O[/tex]
where x and y are the coefficients of the balanced equation. We can use the stoichiometric ratios to set up two equations:
0.180 mol [tex]CO__2[/tex] = x mol [tex]CxHy[/tex] → x = 0.180 mol / 0.0200 mol = 9
0.200 mol [tex]H_2O[/tex] = (y/2) mol [tex]CxHy[/tex] → y = 0.400 mol / 0.0200 mol = 20
Therefore, the molecular formula of the hydrocarbon is [tex]C_9H_20[/tex].
(b) To find the empirical formula of the hydrocarbon, we need to divide the subscripts by their greatest common factor. In this case, both subscripts are divisible by 4, so we get:
[tex]C_9H_20[/tex] → C9/4H5
Therefore, the empirical formula of the hydrocarbon is C9/4H5.
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How does the frequency of a string affect its wavelength?
Answer:
as the frequency goes down, the speed goes down by the same factor, and so the wavelength doesn't change.
Explanation:
Answer: as the frequency goes down, the speed goes down by the same factor, and so the wavelength doesn't change.
Explanation:
The critical point for water lies at 275 °C and 3.2 atm, calculate the DH°vap of water.
The ΔH°vap of water at the critical point is approximately 0.04614 kJ/mol.
To calculate the ΔH°vap (enthalpy of vaporization) of water at the critical point, we can use the Clausius-Clapeyron equation;
ln(P₂/P₁) = ΔH°vap/R [1/T₁ - 1/T₂]
where P₁ and T₁ are the pressure and temperature at which the enthalpy of vaporization is known (usually at standard conditions of 1 atm and 100 °C), P₂ and T₂ are the pressure and temperature at the critical point, ΔH°vap is the enthalpy of vaporization, and R is the gas constant (8.314 J/mol∙K).
Using the given values, we can plug them into the equation and solve for ΔH°vap;
ln(3.2 atm / 1 atm) = ΔH°vap / R [1/373 K - 1/275 K]
Simplifying;
ln(3.2) = ΔH°vap / R [0.0026819]
ΔH°vap / R = ln(3.2) / 0.0026819
ΔH°vap / R = 5.552
Multiplying both sides by R:
ΔH°vap = 5.552 x R
ΔH°vap = 5.552 x 8.314 J/mol∙K
ΔH°vap = 46.14 J/mol
Converting to kJ/mol;
ΔH°vap = 0.04614 kJ/mol
Therefore, the ΔH°vap of water is 0.04614 kJ/mol.
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Write the electronic configuration of all the metal ions in the d-blocks (3d series)
The electronic configuration of the d-block metal ions in the 3d series is represented by electronic configuration of Argon (Ar), 3d and 4s sub orbitals.
What is the electronic configuration of all d block?The electronic configuration of the d-block metal ions in the 3d series is as follows:
Scandium (Sc): [Ar] 3d¹ 4s²
Titanium (Ti): [Ar] 3d² 4s²
Vanadium (V): [Ar] 3d³ 4s²
Chromium (Cr): [Ar] 3d⁵ 4s¹
Manganese (Mn): [Ar] 3d⁵ 4s²
Iron (Fe): [Ar] 3d⁶ 4s²
Cobalt (Co): [Ar] 3d⁷ 4s²
Nickel (Ni): [Ar] 3d⁸ 4s²
Copper (Cu): [Ar] 3d¹⁰ 4s¹
Zinc (Zn): [Ar] 3d¹⁰ 4s²
Thus, the above illustration shows the electronic configuration of all the metal ions in the d-blocks (3d series).
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