Gibbs Free Energy: Equilibrium Constant Nitric oxide, NO, also known as nitrogen

Question

Gibbs Free Energy: Equilibrium Constant Nitric oxide, NO, also known as nitrogen monoxide, is one of the primary contributors to air pollution, acid rain, and the depletion of the ozone layer. The reaction of oxygen and nitrogen to form nitric oxide in an automobile engine is The spontaneity of a reaction can be determined from the free energy change for the reaction, DeltaG degree. A reaction is spontaneous when the free energy change is less than zero. A reaction is nonspontaneous when the free energy change is greater than zero. A reaction is in equilibrium when the free energy change is equal to zero. For the reaction of oxygen and nitrogen to form nitric oxide, consider the following thermodynamic data: Calculate the temperature in kelvins above which this reaction is spontaneous. Express your answer to four significant figures and include the appropriate units. T= 7278 K The standard free energy change. DeltaG degree, and the equilibrium constant K for a reaction can be related by the following equation: where T is the Kelvin temperature and R is equal to 8.314 J/(mol K). Calculate the equilibrium constant for the following reaction at room temperature. 25 degree C: Express your answer numerically to three significant figures.

Explanation / Answer

To calculate the equilibrium constant, let us first calculate the delta Go of the reaction.

   We know delta Go = delta Ho - T. delta So Taking the values from Q1

    delta Go = 180.5 x 1000 J - 298 x 24.80 J = 173109.6 J

now we have delta Go = -2.303RT log K

         173109.6 = -2.303 x8.314 x298 logK

    log K = -30.3389 Or K = 2.182 x 10-30

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