The following reaction was carried out in a 3.75 L reaction vessel at 1100 K: C (s) + H2O (g) ⇌CO (g) + H2 (g) If during the course of the reaction, the vessel is found to contain 6.50 mol of C, 15.9 mol of H2O, 3.20 mol of CO, and 8.20 mol of H2, what is the reaction quotient Q?

The reaction quatient Q is 0.440

Explanation:

Step 1: Data given

Volume = 3.75 L

Temperature = 1100 K

Number of moles of C = 6.50 moles

Number of moles H2O = 15.9 moles

Number of moles CO = 3.20 moles

Number of moles H2 = 8.20

Step 2: The balanced equation

C (s) + H2O (g) ⇌ CO (g) + H2 (g)

Step 3: Calculate the concentration

Concentration = moles / volume

[H2O] = 15.9 moles / 3.75 L

[H2O] = 4.240 M

[CO] = 3.20 moles / 3.75 L

[CO ] = 0.853 M

[H2] = 8.20 moles / 3.75 L

[H2] = 2.187 M

Step 4: Calculate Q

Q = [CO][H2] / [H2O]

Since C (s) is a solid, it doen't affect the reaction qoutient

Q = (0.853 * 2.187) / (4.240)

Q = 0.440

The reaction quatient Q is 0.440

Reaction quotient, Q, is 0.44

Explanation:

For the reaction:

C (s) + H₂O (g) ⇌ CO (g) + H₂ (g)

Reaction quotient Q, at any course of the reaction, is defined as:

Q = [CO][H₂] / [H₂O]

Concentration of reactants is:

[CO] = 3.20mol / 3.75L = 0.853M

[H₂] = 8.20mol / 3.75L = 2.187M

[H₂O] = 15.9mol / 3.75L = 4.24M

Replacing, Q is:

Q = [0.853][2.187] / [4.24]

Q = 0.44