MC+practice

MC+practice - Consider the chemical system CO(g) + Cl2(g)...

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Consider the chemical system CO(g) + Cl 2 (g) COCl 2 (g) K = 4.6 x 10 9 , Δ H = +68 kJ/mol How do the equilibrium pressures of the reactants compare to the equilibrium pressures of the product? a) They are much smaller b) They are much bigger c) They are about the same d) They have to be exactly equal e) You can’t tell from the information given If the concentration of the product were to double, what would happen to the equilibrium constant? a) It would double its value b) It would become half its current value c) It would quadruple its value d) It would not change its value e) It would depend on the initial concentrations of the product Which of the following statements is true? a) If the system is heated, the right side is favored b) This is a heterogeneous equilibrium c) If the pressure is increased by reducing the volume, the left side is favored d) Adding more CO(g) increases the equilibrium constant e) Removing COCl 2 (g) forces equilibrium to the left
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This note was uploaded on 04/25/2008 for the course CHEM 1C taught by Professor Staff during the Spring '01 term at UC Irvine.

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MC+practice - Consider the chemical system CO(g) + Cl2(g)...

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