In a certain reaction 1.5 mol of CO and 1.5 mol of H2O are placed in a 2,0 dm3 sealed vessel. Equilibrium is established at a temperature of 1 000 C. The equilibrium reaction equation is
CO(g) + H2O(g) = CO2(g) + H2(g)
The value of Kc for this reaction is 0,63. Calculate the concetration of CO2 present at equilibriumin the reaction mixture.
To calculate the concentration of CO2 at equilibrium, we need to use the equilibrium constant expression and the given molar amounts of reactants.
First, let's write down the equilibrium constant expression:
Kc = [CO2] * [H2] / [CO] * [H2O]
We are provided with the value of Kc (0.63) and the molar amounts of reactants (1.5 mol of CO and 1.5 mol of H2O). We need to find the concentration of CO2.
Since the volume of the sealed vessel is given as 2.0 dm3, we can assume the total volume of the reaction mixture is 2.0 dm3 as well.
To find the concentration (in mol/dm3) of each substance, we need to divide the moles of each substance by the total volume of the reaction mixture:
[CO] = moles of CO / total volume = 1.5 mol / 2.0 dm3 = 0.75 mol/dm3
[H2O] = moles of H2O / total volume = 1.5 mol / 2.0 dm3 = 0.75 mol/dm3
Since the coefficients of CO and H2O in the balanced equation are both 1, the concentrations of CO and H2O are the same.
Now, let's substitute the known concentrations into the equilibrium constant expression:
0.63 = [CO2] * [H2] / (0.75) * (0.75)
0.63 = [CO2] * [H2] / 0.5625
To find the concentration of CO2, rearrange the equation:
[CO2] = 0.63 * 0.5625 / [H2]
Now, we need to know the concentration of H2. Since we are not given that information, we cannot determine the exact concentration of CO2 at equilibrium without it. The concentration of CO2 depends on the concentration of H2.