At equilibrium a 5000L reaction vessel contains 115 mol of C2H4(aq) and 110 mol of H2)(g) and the Kc = 300.0
The equation for the reaction is:
C2H4(aq) + H2(g) ⇌ C2H6(g)
At equilibrium, the concentrations can be calculated using the ideal gas law:
Kc = [C2H6] / ([C2H4] * [H2])
Given:
- The volume of the reaction vessel is 5000 L.
- The initial moles of C2H4(aq) is 115 mol.
- The initial moles of H2(g) is 110 mol.
- Kc = 300.0.
First, convert the moles of C2H4(aq) and H2(g) to concentrations:
[C2H4] = (moles of C2H4) / (volume of vessel)
= 115 mol / 5000 L
= 0.023 M
[H2] = (moles of H2) / (volume of vessel)
= 110 mol / 5000 L
= 0.022 M
Now substitute these values into the equation for Kc:
300.0 = [C2H6] / (0.023 * 0.022)
Solving for [C2H6]:
[C2H6] = 300.0 * (0.023 * 0.022)
= 0.1512 M
Therefore, at equilibrium, the concentration of C2H6 in the reaction vessel is 0.1512 M.