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13 Dec 2019

1. at 2257 K and 1.00 atm total pressure, water is 1.77 per cent decomposed at equilibrium
by way of the reaction 2 H20(g) = 2 H2(g) + 02(g). Calculate (a) K, (b) ÎrGÎ¦, and (c) ÎrG at this
temperature.
2. on in the Data section. calculate the standard Gibbs energy and the
equilibrium constant at (a) 298 K and (b) 400 K for the reaction PbO(s) + CO(g) = Pb(s) + CO2(g).
Assume that the reaction enthalpy is independent of temperature.
3. Estimate the temperature at which CaC03(calcite) decomposes. The reaction is
CaCO3 (s) ï CaO(s) + CO2(g)
4. when ammonium nitrate undergoes decomposition, only gases are produced,
according to the equation
NH4NO3(s) ï N2O(g) + 2H2O(g)
What is the total volume of gases produced at 546 K and 1.00 atm pressure when 240 g of
ammonium nitrate ( F.W. NH4NO3 = 80) undergoes the above decomposition reaction.
ammonium nitrate ( F.W.

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Casey DurganLv2

17 Dec 2019

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The decomposition of ammonium carbamate (NH4CO2NH2) is described in the reaction below: NH4CO2NH2 (s) 2NH3 (g) + CO2 (g) endothermic reaction A 9.407 g sample of NH4CO2NH2 (s) is placed in an evacuated (ie. initial pressure is 0 atm) 4.000 L vessel at 24Â°C. After equilibrium has been established, the total pressure of the system is 0.318 atm. Some NH4CO2NH2 (s) remains in the vessel. Show work and give answers to the correct number of significant figures.

a) What is the equilibrium partial pressure of NH3 (g) and CO2 (g), respectively?

b) Calculate the KP for the reaction.

c) Calculate the number of moles of NH4CO2NH2 (s) initially. Course: CHEM 1F92 (01, 02) Wednesday, August 31, 2016 Page 5 of 31 Question 2. (continued)

d) Calculate the number of moles of NH3 (g) at equilibrium.

e) What mole fraction of NH4CO2NH2 (s) has been decomposed to NH3 (g)? Report answer in percentage (%).

f) If the volume of the vessel were doubled at constant temperature, which direction would equilibrium shift? Circle the correct answer Shift to Products or Shift to Reactant

g) If the temperature of the system is increased at constant volume, which direction would equilibrium shift? Circle the correct answer. Shift to Products or Shift to Reactant

Q1. Which of the following processes are spontaneous and which are non spontaneous.
a) The combustion of natural gas
b) Extraction of Aluminum metal from its ore
c) A ball rolling down a hill
d) A bike going up a hill

Q2. Predict the entropy change (positive or negative) for the following processes/reactions
a) a lake freezing
b) weeding a garden
c) N2(g) + 2 H2(g) ? N2H4 (g)
d) Mg(s) + 2H2O(l) ? Mg(OH)2 (s) + H2(g)

Q3. The element Cesium (Cs) freezes at 28.4 C and its molar enthalpy of fusion ΔH_fusion = 2.09 kJ/mol.
a) When molten Cs solidifies to Cs (s) at its normal melting point, is the entropy change ΔS positive or negative?
b) Calculate the entropy change S when 15.0 g of Cs(l) solidifies at 28.4 C.

Q4. Using the values for standard molar entropies ΔS_f° from the appendix in your textbook, calculate ΔS° for the following reactions.
a) Be(OH)₂ (s) ? BeO (s) + H2O (g)
b) Mg(OH)2 (s) + 2 HCl (g) ? MgCl2 (s) + 2H2O (l)
c) 2CH4(g) ? C2H6 (g) + H2(g)

Q5. Using the data in the appendix of your textbook, calculate the Gibbs free energy change ΔG° for the following reactions. In each case, indicate whether the reaction is spontaneous or not
a) H2 (g) + Cl2(g) ? 2HCl (g)
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Q6. Consider the reaction 2 NO2 (g)---N2O4 (g)
a) Using the data in the appendix in your text, calculate the standard Gibbs free energy change (ΔG°) for the reaction at 298K.
b) For the above reaction, calculate the value of Keq at 298K
c) For the same reaction, calculate G at 298 K when the partial pressures for NO₂ and N2O4 are 0.40 atm and 0.36 atm, respectively.

Q7. Consider the reaction I2 (g) + Cl2 (g)----2 ICl (g) Kp = 81.9 at 298 K
a) Calculate the standard free energy change (ΔG°)
b) What will be the Free energy change when the above reaction is at equilibrium
c) Calculate G for the reaction at 298 K when PICl = 2.55 atm, PI2=0.325 atm and PCl2 = 0.221 atm

Q8. Consider the decomposition of Lead carbonate PbCO3 (s) ? PbO(s) + CO2 (g)
a) Calculate the Gibbs free energy change (ΔG°) for the reaction at298 K.
b) Calculate G for the reaction at 400 K.
c) Write down the equilibrium expression and calculate the value of Keq at 298 K
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2SO2(g) + O2(g) ? 2SO3(g)

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Q12. What is the minimum temperature required for the spontaneous conversion of CCl4(l) to CCl4(g) when ΔH°(vap) is 57.3 kJ/mol andΔS°(vap) is 164 J/(mol K)? reaction: CCl4(l) ? CCl4(g)

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Fe2O3(s) + 3CO(g) . ? 2Fe(s) + 3CO2(g) ΔG° = 29.4 kJ
3Fe2O3(s) + CO(g) . ? 2Fe3O4(s) + CO2(g) ΔG° = 61.6 kJ
Calculate ΔG° for Fe(s) + Fe2O3(s) + CO2(g) ? Fe3O4(s) +CO(g)

Q14. Calculate ΔG° rxn for 2CO(g) + O2(g) ? 2CO2(g) and then calculate ΔG for the reaction at 298K; if the pressure of CO =20. atm,P O2 = 10. atm and P CO2= 0.50 atm. Will increasing the pressure of the reactants make the reaction more or less spontaneous? Explain using your calculations and Le Chatelierâs principle.

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