Textbook Question
Consider the following equilibrium: 2 H2(g) + S2(g) ⇌ 2 H2S(g) Kc = 1.08 × 107 at 700°C (b) Does the equilibrium mixture contain mostly H2 and S2 or mostly H2S?
16. Chemical Equilibrium
Equilibrium Constant K
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Calculate the equilibrium constant Kc at 304 K for the reaction SO2(g) + Cl2(g) ⇌ SO2Cl2(g) if the equilibrium constant Kp is 33.0 at this temperature.
A
Kc = 0.82
B
Kc = 1.33
C
Kc = 33.0
D
Kc = 40.2
Verified step by step guidance1
Understand the relationship between Kp and Kc. The equilibrium constant Kp is used for reactions involving gases and is expressed in terms of partial pressures, while Kc is expressed in terms of concentrations. The two are related by the equation: , where R is the ideal gas constant, T is the temperature in Kelvin, and Δn is the change in moles of gas.
Calculate Δn for the reaction. Δn is the difference in the number of moles of gaseous products and reactants. For the reaction SO2(g) + Cl2(g) ⇌ SO2Cl2(g), Δn = (moles of products) - (moles of reactants) = 1 - (1 + 1) = -1.
Use the equation relating Kp and Kc: . Rearrange to solve for Kc: .
Substitute the known values into the equation. Use R = 0.0821 L·atm/mol·K for the ideal gas constant and T = 304 K. Substitute Kp = 33.0, R = 0.0821, T = 304, and Δn = -1 into the equation to find Kc.
Perform the calculation to find Kc. This involves evaluating the expression .
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