Question 19 (10 points) Which statement are true in the following choice? Select

Question

Question 19 (10 points)

Which statement are true in the following choice? Select all that apply.

Question 19 options:

Consider the reaction N2 + 3H2 <=> 2NH3

If you start with 1 M concentration of N2 and H2, and x mol/L of N2 are used in the reaction, the concentration of N2 and NH3 at equilibrium are x and 1-x respectively, while the concentration of H2 is 3x.

Consider the reaction N2 + 3H2 <=> 2NH3

If you start with 1 M concentration of N2 and H2, and x mol/L of N2 are used in the reaction, the concentration of N2 and NH3 at equilibrium are 1-x and 2x respectively, while the concentration of H2 is 1-3x.

Given the correct answers to the previous question, the expression of K, the equilibrium constant of the reaction is (2x)^2 / ((1-x) * (1-3x)^3)

Given the correct answers to the previous question, the expression of K, the equilibrium constant of the reaction is (2x) / ((1-x) * (1-3x))

Consider the reaction N2 + 3H2 <=> 2NH3

If you start with 1 M concentration of N2 and H2, and x mol/L of N2 are used in the reaction, the concentration of N2 and NH3 at equilibrium are x and 1-x respectively, while the concentration of H2 is 3x.

Consider the reaction N2 + 3H2 <=> 2NH3

If you start with 1 M concentration of N2 and H2, and x mol/L of N2 are used in the reaction, the concentration of N2 and NH3 at equilibrium are 1-x and 2x respectively, while the concentration of H2 is 1-3x.

Given the correct answers to the previous question, the expression of K, the equilibrium constant of the reaction is (2x)^2 / ((1-x) * (1-3x)^3)

Given the correct answers to the previous question, the expression of K, the equilibrium constant of the reaction is (2x) / ((1-x) * (1-3x))

Explanation / Answer

A. N2 + 3H2 <=> 2NH3

If you start with 1 M concentration of N2 and H2, and x mol/L of N2 are used in the reaction, the concentration of N2 and NH3 at equilibrium are x and 1-x respectively, while the concentration of H2 is 3x.

FALSE : the cncentration of H2 will be 1-3x and NH3 will be 2x as   

   N2 + 3H2 <=> 2NH3

at t = 0 1M 1M 0M

at t = t 1-x 1-3x 0 +2x (conc of reactants is used up therefore minus, and conc of products added)

so, the statement is FALSE.

B. If you start with 1 M concentration of N2 and H2, and x mol/L of N2 are used in the reaction, the concentration of N2 and NH3 at equilibrium are 1-x and 2x respectively, while the concentration of H2 is 1-3x

FALSE: as seen above, the concentration of NH3 will be 2x. So, the statement is FALSE.

C. Given the correct answers to the previous question, the expression of K, the equilibrium constant of the reaction is (2x)^2 / ((1-x) * (1-3x)^3)

TRUE: at equilibrium, K = [NH3]2/ [N2][H2]3

D. Given the correct answers to the previous question, the expression of K, the equilibrium constant of the reaction is (2x) / ((1-x) * (1-3x))

FALSE: the correct equilibrium constant is represented by (2x)^2 / ((1-x) * (1-3x)^3) .

THE CORRECT STATEMENT IS Given the correct answers to the previous question, the expression of K, the equilibrium constant of the reaction is (2x)^2 / ((1-x) * (1-3x)^3)

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