6) McQuarrie & Simon, Problems 26.16 & 26.17: Consider the following two chemica

Question

6) McQuarrie & Simon, Problems 26.16 & 26.17: Consider the following two chemical equations co(g) + H2O(g) CO2(g)+H2(g): CH,(g) + H20(g) C0(g)+3H2(g): a) Show that if we were to add these two chemical equations to form a third equation, the with equilibrium constants Ki and K2: K1 K2 equilibrium constant of the combined equation, K3, is equal to the product of K and K2 How do you explain that you add the values of AG" but multiply the equilibrium constants when combining equations 1 and 2 to form a new chemical equation? Consider the following two exchange reactions: b) c) 2BrCI(g) Cl2(g)+Br(g): KP = 0.169 2/Br(g) Br(g) +1,(g): KP 0.0149 Using the strategy you employed in part a above, determine the value of Kp for the following reaction:

Explanation / Answer

C)

from the given equations

   1/2* (2BrCl(g) <===> Cl2(g) + Br2(g))   Kp1 = 0.169^(1/2)

    1/2*( I2 + Br2 <===> 2IBr(g))         Kp2 = (1/(0.0149)^(1/2)
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BrCl(g) + 1/2 Br2 <===> IBr(g) + 1/2Cl2(g) Kp = Kp1*Kp2
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   Kp = 0.169^(1/2)*(1/0.0149)^(1/2)

      = 3.37

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