find eq constant at 910K. CCl4 (g)--> <--CCl4(l)
given: Gf CCl4(g)= -53.7
Gf CCl4(l)= -68.6
G Products - G reactants = Delta G.
Delta G = -RT ln Keq
To find the equilibrium constant (Keq) at a given temperature (910K) for the reaction CCl4 (g) ⇌ CCl4 (l), we can use the formula:
Delta G = -RT ln Keq
G Products - G Reactants = Delta G
First, let's calculate Delta G using the given values for the standard Gibbs free energy of formation (Gf):
Gf CCl4(g) = -53.7
Gf CCl4(l) = -68.6
Delta G = G Products - G Reactants
= Gf CCl4(l) - Gf CCl4(g)
= -68.6 - (-53.7)
= -14.9
Now, we can substitute the values into the formula and solve for Keq:
-14.9 = -RT ln Keq
Since the temperature is given as 910K and R is the gas constant (8.314 J/(mol·K)), we can substitute these values:
-14.9 = -(8.314)(910) ln Keq
Now, we can solve for ln Keq:
ln Keq = -14.9 / (8.314 × 910)
Finally, we can solve for Keq by taking the exponential of both sides:
Keq = e^(ln Keq)
Therefore, Keq at 910K for the given reaction is the exponential of the calculated value of ln Keq.