The equilibrium constant for the following reaction is 1.89×10-2 at 444 °C. 2 HI (g) ------> <----------- H2  (g) + I2 (g)        K =1.89×10-2 at 444 °C Calculate the equilibrium constant for the following reactions at 444 °C. (a)   H2(g) + I2(g)  2 HI(g)       K = _____________ (b)   HI(g)  1/2 H2(g) + 1/2 I2(g)       K = ____________ B2: The following gas phase system is at equilibrium, CCl4(g) + CH4(g) ⇄ 2 CH2Cl2(g) The pressures of each gas measured are: PCCl4 = 198 mmHg PCH4 = 0.337 mmHg PCH2Cl2 = 135 mmHg What is the value of the equilibrium constant in terms of pressures, Kp?

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