Multiple Choice
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)?
16. Chemical Equilibrium
Equilibrium Constant Calculations
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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?
A
2.10 M
B
2.53 M
C
0.83 M
D
2.10 M
Verified step by step guidance1
Understand the equilibrium expression for the reaction CO2(g) ⇌ CO2(aq). The equilibrium constant Kc is given for the concentration of CO2 in the aqueous phase relative to the gaseous phase.
The equilibrium constant Kc is defined as the ratio of the concentration of the products to the concentration of the reactants. For this reaction, Kc = [CO2(aq)] / [CO2(g)].
Since Kc is given as 0.83 and the partial pressure of CO2(g) is 2.53 atm, we need to convert the partial pressure to concentration using the ideal gas law. The formula is: \( [CO2(g)] = \frac{P}{RT} \), where P is the pressure, R is the ideal gas constant, and T is the temperature in Kelvin.
Assuming standard conditions (T = 298 K and R = 0.0821 L·atm/mol·K), calculate the concentration of CO2(g) using the ideal gas law: \( [CO2(g)] = \frac{2.53}{0.0821 \times 298} \).
Finally, use the equilibrium expression to solve for the concentration of CO2(aq): \( [CO2(aq)] = Kc \times [CO2(g)] \). Substitute the values to find the concentration of CO2(aq).
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