Question

What is the pressure of CO2 in a mixture at equilibrium that contains 0.50 atm H2, 2.0 atm of H2O, and 1.0 atm of CO at 990 °C?

a) 0.75 atm
b) 1.50 atm
c) 2.25 atm
d) 3.00 atm

Answer 1

To find the pressure of CO2 in the mixture at equilibrium, calculate the number of moles of each component in the mixture and subtract the pressures of the other components from the total pressure.

Step-by-step explanation:

To determine the pressure of CO2 in the mixture at equilibrium, you need to calculate the number of moles of each component using the given information. From the balanced chemical equation H₂(g) + CO₂(g) = H₂O(g) + CO(g), we know that the stoichiometric ratio between H2 and CO2 is 1:1. Therefore, the number of moles of CO2 in the mixture is also 1.0 mole.

Since the total pressure in the mixture is given as 0.50 atm H2 + 2.0 atm H2O + 1.0 atm CO, the total pressure is 0.50 + 2.0 + 1.0 = 3.50 atm. Since the pressure of CO2 can be obtained by subtracting the pressures of the other components from the total pressure, the pressure of CO2 in the mixture at equilibrium is 3.50 atm - 0.50 atm - 2.0 atm = 1.0 atm.