Chemical Equilibrium Constant Calculation

AI Thread Summary
To calculate the equilibrium constant (Keq) for the reaction C(s) + O2(g) → CO2(g) at 25°C, the relationship between Gibbs free energy change (dGorxn) and Keq is essential. The provided Gibbs free energy of formation for CO2 is -394.36 kJ/mol, while the values for C(s) and O2(g) are zero. The equation dGorxn = -R*T*ln(Keq) is used, but the user initially calculated an incorrect value for Keq. Clarification on the significance of the reaction quotient (Q) and its relationship to Keq is also sought, indicating confusion about the concepts involved.
hotwheelharry
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Homework Statement



If Q = 1.0 1042 for the reaction C(s) + O2(g) → CO2(g) at 25°C, calculate Keq.

dGof (Kj/mol) of...
C(s)=0
O2(g)=0
CO2(g)=-394.36

Homework Equations


dGorxn = -R*T*ln(K)

The Attempt at a Solution



-394.36*1000 = -8.314472(298)ln(K)
K=1.3e69

This is the wrong answer. I'm lost as to what to do. Please help.
I might be using the wrong equation for the situation. The only information I was given was in the problem statement.
 
Last edited:
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What is Q? How is it related to Keq?
 
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