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At 700 K the equilibrium constant for the reaction CCl4(g) <===> C(s) + 2 Cl2(g) is Kp = 0.76. A flask is charged with 2.00 atm CCl4, which then reaches equilibrium at 700 K.
(a) What fraction of the CCl4 is converted into C and Cl2;
(b) What are the partial pressures of CCl4 and Cl2 at equilibrium?
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Consider the following reaction: CO(g)+H2O(g)in equilibrium with CO2(g)+H2
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At a certain temperature the equilbrium constant is 396 K for H2(g) + I2(g) ↔ 2HI(g) , Calculate the the equilbrium constant for 0.5H2(g) + 0.5I2(g) ↔ HI(g)
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