Question

1. Write the equilibrium constant expressions for the following equilibria: i) H2CO3(aq) ? 2H+(aq) + CO32-(aq) ii) H2(g) + I2(g) ? 2HI(g) iii) H2O(aq) + Cl2(aq) ? HCl(aq) + HOCl(aq) iv) 2NO(g) + O2(g) ? 2NO2(g) 2. During the Contact Process SO3 is produced from SO2 in a reversible reaction: 2SO2(g) + O2(g) ? 2SO3(g) i) Write an expression for the equilibrium constant, Kc, and derive its units. ii) When the equilibrium was established at 1000K; the following concentrations were found: 1.00 moldm-3 SO2 0.2 moldm-3 O2 1.3 moldm-3 SO3 Calculate Kc at this temperature. iii) What does the magnitude of Kc tell you about the proportion of reactants to products at equilibrium? Explain your answer. 3. CH4(g) + 2 H2O(g) ? CO2(g) + 4H2(g) T = 298K Analysis of this equilibrium mixture gave the following results: 0.0800 moldm-3 CH4 0.320 moldm-3 H2O 0.200 moldm-3 CO2 0.280 moldm-3 H2 iv) Write the equilibrium constant expression for this equilibrium; calculate the value of Kc including units. v) What does the magnitude of Kc tell you about the proportion of reactants to products at equilibrium? Explain your answer. vi) How would the value of Kc change if a catalyst was added? Explain your answer.

          1. Write the equilibrium constant expressions for the following equilibria:
i) H2CO3(aq) ? 2H+(aq) + CO32-(aq)
ii) H2(g) + I2(g) ? 2HI(g)
iii) H2O(aq) + Cl2(aq) ? HCl(aq) + HOCl(aq)
iv) 2NO(g) + O2(g) ? 2NO2(g)

2. During the Contact Process SO3 is produced from SO2 in a reversible reaction:
2SO2(g) + O2(g) ? 2SO3(g)

i) Write an expression for the equilibrium constant, Kc, and derive its units.
ii) When the equilibrium was established at 1000K; the following concentrations were found:
1.00 moldm-3 SO2
0.2 moldm-3 O2
1.3 moldm-3 SO3
Calculate Kc at this temperature.
iii) What does the magnitude of Kc tell you about the proportion of reactants to products at equilibrium? Explain your answer.

3. CH4(g) + 2 H2O(g) ? CO2(g) + 4H2(g) T = 298K
Analysis of this equilibrium mixture gave the following results:
0.0800 moldm-3 CH4
0.320 moldm-3 H2O
0.200 moldm-3 CO2
0.280 moldm-3 H2
iv) Write the equilibrium constant expression for this equilibrium; calculate the value of Kc including units.
v) What does the magnitude of Kc tell you about the proportion of reactants to products at equilibrium? Explain your answer.
vi) How would the value of Kc change if a catalyst was added? Explain your answer.

1. Write the equilibrium constant expressions for the following equilibria:
i) H2CO3(aq) ? 2H+(aq) + CO32-(aq)
ii) H2(g) + I2(g) ? 2HI(g)
iii) H2O(aq) + Cl2(aq) ? HCl(aq) + HOCl(aq)
iv) 2NO(g) + O2(g) ? 2NO2(g)

2. During the Contact Process SO3 is produced from SO2 in a reversible reaction:
2SO2(g) + O2(g) ? 2SO3(g)

i) Write an expression for the equilibrium constant, Kc, and derive its units.
ii) When the equilibrium was established at 1000K; the following concentrations were found:
1.00 moldm-3 SO2
0.2 moldm-3 O2
1.3 moldm-3 SO3
Calculate Kc at this temperature.
iii) What does the magnitude of Kc tell you about the proportion of reactants to products at equilibrium? Explain your answer.

3. CH4(g) + 2 H2O(g) ? CO2(g) + 4H2(g) T = 298K
Analysis of this equilibrium mixture gave the following results:
0.0800 moldm-3 CH4
0.320 moldm-3 H2O
0.200 moldm-3 CO2
0.280 moldm-3 H2
iv) Write the equilibrium constant expression for this equilibrium; calculate the value of Kc including units.
v) What does the magnitude of Kc tell you about the proportion of reactants to products at equilibrium? Explain your answer.
vi) How would the value of Kc change if a catalyst was added? Explain your answer.

Added by John J.

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