Question

Calculate the pressure of H2 (in atm) required to maintain equilibrium with respect to the following reaction at 25°C:

Pb(s) + 2H(aq) ⇌ Pb_2(aq) + H_2(g)
Given that [Pb2]=0.035M and the solution is buffered at pH 1.60.
a. 0.025 atm
b. 0.050 atm
c. 0.075 atm
d. 0.100 atm

Answer 1

To calculate the pressure of H2 required to maintain equilibrium with respect to the given reaction, we need to use the equilibrium constant expression and rearrange it to solve for [H2].

Step-by-step explanation:

To calculate the pressure of H2 required to maintain equilibrium with respect to the given reaction, we need to use the equilibrium constant expression.

The equilibrium constant (K) for the reaction is defined as the ratio of the product concentrations to the reactant concentrations, each raised to their stoichiometric coefficients. In this case, the equilibrium constant expression is:

K = [Pb2+][H2] / [Pb][H+]

Given that [Pb2+] = 0.035M, the equilibrium constant can be rearranged to solve for [H2].

Using the given equilibrium concentration and the equilibrium constant expression, we can calculate the pressure of H2 required to maintain equilibrium.