The equilibrium constant, K_c, is calculated using molar concentrations. For gas

Question

The equilibrium constant, K_c, is calculated using molar concentrations. For gaseous reactions another form of the equilibrium constant, K_p, is calculated from partial pressures instead of concentrations. These two equilibrium constants are related by the equation K_p = K_c (RT)^Delta n where R = 0.08206 L atm/(K mol), T is the absolute temperature, and Delta n is the change in the number of moles of gas (sum moles products - sum moles reactants). For example, consider the reaction N_2(g) + 3H_2(g) = 2NH_3(g) for which Delta n = 2 - (1 + 3) = -2. For the reaction 3A(g) + 2B(g) = c(g) K_c = 88.8 at a temperature of 325 degree C Calculate the value of K_p. For the reaction X(g) + 3Y(g) = 2Z(g) K_p = 1.33 Times 10^-2 at a temperature of 31 degree C . Calculate the value of K_c.

Explanation / Answer

Part A:

Dn= 1 - (3 + 2)= -4

Kp= 88.8 (0.08206 x 598K)-4= 1.53 x10-5

Part B:

Dn= 2 - (3 + 1)= -2

1.33x10-2=Kc (0.08206 x 304)-2 ----> Kc= 8.28

The first one was a math mistake, but the second one is still ok for me, i can´t find the mistake

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