The Reaction Quotient Video Lessons

Example

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:

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.