Hey im stumped on this sheet :) 1.If the equilibrium constant, Keq, for the conversion of isobutene to n-butane is 2.5, what is the valueof the equilibrium constant for the reverse reaction?b. 0.4a. 2.5e. 1.02.Which of the following affect the value of the equilibrium constant?a. temperatureb. small changes in concentrationc. the density of a slightly soluble saltc. 6.25PC15(g) + 45 kJd. small changes in the pressure of a gase. both (a) and (b)3.For the equilibrium system below, which of the following would result in an increase in the quantityof PC15(g)?d. 1.3PC13(g) + Cl2(g)a. increasing temperatured. removing some Cl₂(g)b. increasing the size of the container e. injecting some He gasc. decreasing temperature4.If sulfur trioxide (gas) is bubbled into water (liquid), concentrated sulfuric acid is produced. Thisequilibrium has a very large K value and is very exothermic. What do these facts indicate?H₂(g) + I₂(g)2HI(g) + 65 kJa. 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.

Dear student , since you have posted multiple questions we are allowed to solve only first question…

Answered: If the equilibrium constant, Keq, for…

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

Chemistry & Chemical Reactivity

9th Edition

ISBN:9781133949640

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter18: Principles Of Chemical Reactivity: Entropy And Free Energy

Section: Chapter Questions

Problem 67SCQ

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Question

Hey im stumped on this sheet :)

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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