Question

The following reaction was carried out in a 3.25 L reaction vessel at 1100 K:


`C(s) + H_2O(g) \rightleftharpoons CO(g) + H_2(g)`
If during the course of the reaction, the vessel is found to contain 5.25 mol of C, 13.3 mol of H₂O, 3.40 mol of CO, and 6.30 mol of H₂, what is the reaction quotient Q?
Enter the reaction quotient numerically.

Answer 1

Answer : The value of reaction quotient Q is, 0.498

Step-by-step explanation:

Reaction quotient (Q) : It is defined as the measurement of the relative amounts of products and reactants present during a reaction at a particular time.

The given balanced chemical reaction is,

`C(s)+H_2O(g)\rightarrow CO(g)+H_2(g)`

The expression for reaction quotient will be :

`Q=([CO][H_2])/([H_2O])`

In this expression, only gaseous or aqueous states are includes and pure liquid or solid states are omitted.

Now we have to calculate the concentration of
`H_2O,CO\text{ and }H_2`

`\text{Concentration of }H_2O=\frac{\text{Moles of }H_2O}{\text{Volume of solution}}=(13.3mol)/(3.25L)=4.09M`

and,

`\text{Concentration of }CO=\frac{\text{Moles of }CO}{\text{Volume of solution}}=(3.40mol)/(3.25L)=1.05M`

and,

`\text{Concentration of }H_2=\frac{\text{Moles of }H_2}{\text{Volume of solution}}=(6.30mol)/(3.25L)=1.94M`

Now put all the given values in the above expression, we get:

`Q=((1.05)* (1.94))/((4.09))=0.498`

Thus, the value of reaction quotient Q is, 0.498