Background: The equilibrium constant, Kc, is calculated using molar concentratio

Question

Background: 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)+2B(g)C(g) Kc = 92.2 at a temperature of 237 C . Calculate the value of Kp.

Part B: For the reaction X(g)+3Y(g)2Z(g) Kp = 3.61×102 at a temperature of 79 C . Calculate the value of Kc.

Explanation / Answer

Part A:- n = 1 - ( 2 + 2) = -3

Kp = 92.2 x ( 0.08206 x 510)-3

Kp = 1.258 x 10-3

Part B:-  n = 2 - (3 + 1) = -2

  3.61×102 = Kc (0.08206 x 352 )-2

Kc = 4.326 x 10-5

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