Pressure -Based versus Concentration- Based Equilibrium Constants The equilibriu

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)^delta n where R = 0.082.06 L . atm/(K . mol), T is the absolute temperature, and delta n is the change in the number of moles of gas. For example, consider the reaction N2 (g) + 3H2(g) 2NH3(g) for which delta n = 2 - (1 + 3) = -2 Part A For the reaction 3A(g) + 2B(g) C(g) Kc = 71.6 at a temperature of 185 degree C. Calculate the value of Kp. Express your answer numerically. Kp = Part B For the reaction X(g) + 2Y(g) 2Z(g) Kp = 3.35x10^-2 at a temperature of 139 degree C. Calculate the value of Kc. Express your answer numerically. Kc =

Explanation / Answer

PART-A

Kp= Kc(RT)^n

n = 1-(2+3)

n= -4

Kp = 71.6*(0.08206*458)^-4

Kp=3.588*10^-5

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PART-B

Kp= Kc(RT)^n

n= 2-(1+2)

n=-1

3.35*10^-2= Kc(0.08206*412)^-1

3.35*10^-2 = 0.02957*Kc

Kc= 1.1325

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