CHEMITRY HELP!!! Gibbs Free Energy: Equilibrium Constant!!? |

CHEMITRY HELP!!! Gibbs Free Energy: Equilibrium Constant!!?

August 18th, 2010

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Calculate the equilibrium constant for the reaction of nitric oxide formation at room temperature, 25 degrees C. The reaction N2 (g) + O2 (g )—> 2NO (g). Gf Delta NO (g) is 87. 6 kJ / molGf delta for both O2 and N2 gas is equal to zero delta G is just 2 * 87. 6 * 1000 = 175200JJ’ai used the formula =- deltaG RTlnK and solved for K.175200J / – (8. 314 * 298) = e ^ I did lnkPuis 175200J / – (8. 314 * 298)) = K but I K = 1. 95 × 10 ^ -31, but its telling me that it is wrong. Can anyone tell me where I am wrong. Someone please help me!

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One Response to “CHEMITRY HELP!!! Gibbs Free Energy: Equilibrium Constant!!?”

Dartanian says:

August 18, 2010 at 2:54 am

You are setting it up correctly, but delta G should be rounded off to 1.73×10^5 J, instead of 1.752 ×10^5 J.

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