The following reaction was carried out in a 2.00 reaction vessel at 1100 :
C+H2O -> C)+H2
If during the course of the reaction, the vessel is found to contain 7.00mol of C, 13.3mol of H2o, 3.80mol of CO, and 7.20mol of H2, what is the reaction quotient ?
Enter the reaction quotient Q?
To calculate the reaction quotient (Q), we need to determine the concentrations of the reactants and products at a given point in the reaction. The reaction quotient is calculated in the same way as the equilibrium constant (K), but it can be calculated at any point during the reaction, not just at equilibrium.
Given:
- Initial moles of C (carbon) = 7.00 mol
- Initial moles of H2O (water) = 13.3 mol
- Moles of CO (carbon monoxide) formed = 3.80 mol
- Moles of H2 formed = 7.20 mol
Since the reaction is balanced:
C + H2O -> CO + H2
From the balanced equation, we can see that the stoichiometric ratio between C and CO is 1:1, and between H2O and H2 is also 1:1.
So, based on the given information, we can determine the concentrations as follows:
Concentration of C = (moles of C) / (volume of the reaction vessel)
Concentration of C = 7.00 mol / 2.00 L = 3.50 M
Concentration of H2O = (moles of H2O) / (volume of the reaction vessel)
Concentration of H2O = 13.3 mol / 2.00 L = 6.65 M
Concentration of CO = (moles of CO) / (volume of the reaction vessel)
Concentration of CO = 3.80 mol / 2.00 L = 1.90 M
Concentration of H2 = (moles of H2) / (volume of the reaction vessel)
Concentration of H2 = 7.20 mol / 2.00 L = 3.60 M
Now we can write the reaction quotient (Q) using the concentrations:
Q = ([CO]^a * [H2]^b) / ([C]^c * [H2O]^d)
From the balanced equation:
a = 1 (coefficient of CO)
b = 1 (coefficient of H2)
c = 1 (coefficient of C)
d = 1 (coefficient of H2O)
Therefore:
Q = ([CO]^1 * [H2]^1) / ([C]^1 * [H2O]^1)
Q = (1.90 * 3.60) / (3.50 * 6.65)
Calculating this expression will give you the reaction quotient Q.