16. Chemical Equilibrium

Given the equilibrium reaction 2CO(g) + O2(g) ⇌ 2CO2(g) with Kc = 2.8 × 10^2 at 298 K, and the partial pressures of CO and O2 are 5.168 × 10^-8 torr and 0.988 torr respectively, what is the partial pressure of CO2 in this mixture?

Given the following reactions and their equilibrium constants, calculate the equilibrium constant (Kc) for the reaction: 2A(g) + B(g) ⇌ A2B(g). Reaction 1: A2B(g) + B(g) ⇌ A2B2(g), Kc = 16.4 Reaction 2: 2A(g) + 2B(g) ⇌ A2B2(g), Kc = 28.2

In a solution at equilibrium with both PbSO4 and SrSO4, what is the relationship between the concentrations of [SO4^2-], [Pb^2+], and [Sr^2+]?

Consider the reaction C2H4(g) + H2O(g) -> CH3CH2OH(g). Using the standard thermodynamic data, calculate the equilibrium constant (K) for this reaction at 298.15 K.

Given the reaction Fe²⁺(aq) + Mn(s) ⇌ Fe(s) + Mn²⁺(aq), calculate the equilibrium constant (K) at 25°C if the concentrations at equilibrium are [Fe²⁺] = 0.010 M and [Mn²⁺] = 0.020 M. Express your answer to two significant figures.

Hydrogen peroxide decomposes according to the equation 2H2O2(l) → 2H2O(l) + O2(g). Calculate Kp for this reaction at 25°C given ΔH° = -98.2 kJ/mol and ΔS° = 70.1 J/K·mol.

At a certain temperature, the equilibrium constant, Kc, equals 0.11 for the reaction: 2 ICl(g) ⇌ I2(g) + Cl2(g). What is the equilibrium concentration of ICl if 0.45 mol of I2 and 0.45 mol of Cl2 are initially mixed in a 2.0-L flask?

Cyclohexane, C6H12, undergoes a molecular rearrangement in the presence of AlCl3 to form methylcyclopentane, CH3C5H9, according to the equation: C6H12 ⇌ CH3C5H9. If Kc = 0.143 at 25°C for this reaction and the initial concentration of C6H12 is 1.0 M with no CH3C5H9 present initially, what are the equilibrium concentrations of C6H12 and CH3C5H9?

An equilibrium mixture of CO, O2, and CO2 at a certain temperature contains 0.0010 M CO2 and 0.0020 M O2. At this temperature, Kc equals 1.4 × 10^2 for the reaction: 2 CO(g) + O2(g) ⇌ 2 CO2(g). What is the equilibrium concentration of CO?

The equilibrium constant for the reaction 2NO(g) + Br2 ⇌ 2NOBr(g) is Kc = 2.0 × 10⁻² at a certain temperature. Calculate Kc for the reverse reaction NOBr(g) ⇌ NO(g) + 1/2Br2(g).

Kc is 1.67 × 10^20 at 25°C for the formation of iron(III) oxalate complex ion: Fe3+(aq) + 3 C2O4^2-(aq) ⇌ [Fe(C2O4)3]^3-(aq). If 0.0100 M Fe3+ is initially mixed with 1.00 M oxalate ion, what is the concentration of Fe3+ ion at equilibrium?

Cyclohexane, C6H12, undergoes a molecular rearrangement in the presence of AlCl3 to form methylcyclopentane, CH3C5H9, according to the equation: C6H12 ⇌ CH3C5H9. If Kc = 0.143 at 25°C for this reaction and the initial concentration of C6H12 is 1.0 M with no CH3C5H9 present initially, what are the equilibrium concentrations of C6H12 and CH3C5H9?

Consider the following reaction: 2 H2O(g) + 2 SO2(g) ⇌ 2 H2S(g) + 3 O2(g). A reaction mixture initially contains 2.8 M H2O and 2.6 M SO2. Determine the equilibrium concentration of H2S if Kc for the reaction at this temperature is 1.3 × 10^-6.

What is the concentration of aqueous CO2 in the reaction CO2(g) ⇌ CO2(aq) with a Kc of 0.83, given the partial pressure of CO2(g) is 2.53 atm?

Given the equilibrium constant for the reaction H2(g) + Br2(g) ⇌ 2 HBr(g) is Kc = 3.8 × 10^4, what is the equilibrium constant for the reverse reaction 4 HBr(g) ⇌ 2 H2(g) + 2 Br2(g)?