Pressure-Based versus Concentration-Based Equilibrium Constants The equilibrium

Question

Pressure-Based versus Concentration-Based Equilibrium Constants The equilibrium constant, Kc, is calculated using molar concentrations. For gaseous reactions another form of the equilibrium constant, Kp, is calculated from partial pressures instead of concentrations. These two equilibrium constants are related by the equation Kp=Kc(RT)n where R=0.08206 Latm/(Kmol), T is the absolute temperature, and n is the change in the number of moles of gas (sum moles products - sum moles reactants). For example, consider the reaction N2(g)+3H2(g)2NH3(g) for which n=2(1+3)=2.

Part A

For the reaction 2A(g)+3B(g)C(g) Kc = 64.8 at a temperature of 107 C . Calculate the value of Kp. Express your answer numerically.

Part Part B

For the reaction X(g)+2Y(g)3Z(g) Kp = 2.77×102 at a temperature of 337 C . Calculate the value of Kc. Express your answer numerically.

Explanation / Answer

Part A

Kc=64.8

T=107+273=380K

Kp=Kc×(RT)^dn

Kp=64.8×(0.08206×380)^(-4)

Kp=6.84×10^-5

PartB

Kp=2.77×10^-2

T=337+273=610K

Kc=Kp×(RT)^-dn

Kc=(2.77×10^-2)×(0.08206×610)^-(0)

Kc=2.77×10^-2

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