equilibrium - Equilibrium 1. For a chemical reaction at...

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Equilibrium 1. For a chemical reaction at equilibrium, the relationship between the rate constants for the forward and reverse reactions (k f and k r ) and the equilibrium constant for the process (K eq ) is B A f r k k A. K eq = k f k r B. K eq = k f - k r C. K eq = k f + k r D. K eq = k f / k r E. K eq = k r / k f 2. Which of the following will change the value of an equilibrium constant? 1. changing temperature 2. adding a catalyst 3. varying the initial concentration of reactants A. 1 only B. 2 only C. 1 and 2 D. 1 and 3 E. all three 3. K c for the reaction HCl(g) + NH 3 (g) NH 4 Cl(s) is A. [] [] [ ] 3 4 NH HCl Cl NH B. [] [ [] ] Cl NH NH HCl 4 3 C. [] [ ] 3 NH HCl 1 D. [HCl] [NH 3 ] E. [NH 4 Cl]
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4. Consider the following three reactions: 1. H 2 (g) + Cl 2 (g) 2 HCl(g) 2. C(s) + H 2 O(g) CO(g) + H 2 (g) 3. Fe 3 O 4 (s) + 4H 2 (g) 3 Fe(s) + 4H 2 O(g) For which of these would K p = K c ? A. 1 only B. 1 and 2 only C. 1 and 3 only D. 3 only E. 2 and 3 only 5. At 50 ° C, K c = 2.2 × 10 3 for the reaction 3 Fe(s) + 4 H 2 O(g) Fe 3 O 4 (s) + 4 H 2 (g) What is the value of K p at 200 ° C for this reaction? A. 8.8 × 10 3 B. 2.2 × 10 3 C. 5.5 × 10 2 D. 3.5 × 10 4 E. This question cannot be answered with the information provided 6. For the following reaction, K p = 1.96 at 700 K. NOCl(g)
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equilibrium - Equilibrium 1. For a chemical reaction at...

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