# Problem: The water-gas shift reaction is an extremely important one in industry.CO(g) + H2O(g) &lt;=&gt; CO2(g) + H2(g)At a given temperature, Kp =2.7. If 0.54 moles of CO, 0.22 moles of H2O, 1.02 moles of CO2 and 0.11 moles of H2 are placed in a 2.0 L flask, thenA. Q = 1.05, reaction will go to the rightB. Q = 0.94, reaction will go to the rightC. Q = 1.05, reaction will go to the leftD. Q = 0.94, reaction will go to the leftE. The reaction is at equilibrium.

###### FREE Expert Solution

We are being asked what would be the reaction condition of the reaction mixture given the concentrations of the reactants and product. We're given the following reaction:

CO(g) + H2O(g) ⇌ CO2(g) + H2(g)

We will use the reaction quotient, Q, to determine if a chemical reaction would be at equilibrium or not. The formula for Q is:

$\overline{){\mathbf{Q}}{\mathbf{=}}\frac{\mathbf{products}}{\mathbf{reactants}}}$

At a given temperature, the Kp for this reaction is 2.7. Depending on if Q is greater than or less than K our reaction will shift to attain equilibrium by reaching the equilibrium constant K:

91% (110 ratings) ###### Problem Details

The water-gas shift reaction is an extremely important one in industry.

CO(g) + H2O(g) <=> CO2(g) + H2(g)

At a given temperature, Kp =2.7. If 0.54 moles of CO, 0.22 moles of H2O, 1.02 moles of CO2 and 0.11 moles of H2 are placed in a 2.0 L flask, then

A. Q = 1.05, reaction will go to the right

B. Q = 0.94, reaction will go to the right

C. Q = 1.05, reaction will go to the left

D. Q = 0.94, reaction will go to the left

E. The reaction is at equilibrium.