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If the equilibrium constant, Keq, for the conversion of isobutene to n-butane is 2.5, what is the value of the equilibrium constant for the reverse reaction? a. 2.5 e. 1.0 b. 0.4 c. 6.25 d. 1.3

If the equilibrium constant, Keq, for the conversion of isobutene to n-butane is 2.5, what is the value of the equilibrium constant for the reverse reaction? a. 2.5 e. 1.0 b. 0.4 c. 6.25 d. 1.3

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Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
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1. If the equilibrium constant, Keq, for the conversion of isobutene to n-butane is 2.5, what is the value of the equilibrium constant for the reverse reaction? b. 0.4 a. 2.5 e. 1.0 2. Which of the following affect the value of the equilibrium constant? a. temperature b. small changes in concentration c. the density of a slightly soluble salt c. 6.25 PC15(g) + 45 kJ d. small changes in the pressure of a gas e. both (a) and (b) 3. For the equilibrium system below, which of the following would result in an increase in the quantity of PC15(g)? d. 1.3 PC13(g) + Cl2(g) a. increasing temperature d. removing some Cl₂(g) b. increasing the size of the container e. injecting some He gas c. decreasing temperature 4. If sulfur trioxide (gas) is bubbled into water (liquid), concentrated sulfuric acid is produced. This equilibrium has a very large K value and is very exothermic. What do these facts indicate? H₂(g) + I₂(g) 2HI(g) + 65 kJ a. Very little product is formed. b. The temperature increase would drive the reaction to the left. c. This is not a spontaneous reaction. d. The reaction is spontaneous, and the equilibrium position is to the far right. e. All of the above apply.
Transcribed Image Text:1. If the equilibrium constant, Keq, for the conversion of isobutene to n-butane is 2.5, what is the value of the equilibrium constant for the reverse reaction? b. 0.4 a. 2.5 e. 1.0 2. Which of the following affect the value of the equilibrium constant? a. temperature b. small changes in concentration c. the density of a slightly soluble salt c. 6.25 PC15(g) + 45 kJ d. small changes in the pressure of a gas e. both (a) and (b) 3. For the equilibrium system below, which of the following would result in an increase in the quantity of PC15(g)? d. 1.3 PC13(g) + Cl2(g) a. increasing temperature d. removing some Cl₂(g) b. increasing the size of the container e. injecting some He gas c. decreasing temperature 4. If sulfur trioxide (gas) is bubbled into water (liquid), concentrated sulfuric acid is produced. This equilibrium has a very large K value and is very exothermic. What do these facts indicate? H₂(g) + I₂(g) 2HI(g) + 65 kJ a. Very little product is formed. b. The temperature increase would drive the reaction to the left. c. This is not a spontaneous reaction. d. The reaction is spontaneous, and the equilibrium position is to the far right. e. All of the above apply.
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