I don't understand this concenpt. I know Q= 77.44 and K=9.60, Q > K which means reactants are already favored, so why is the answer "more nitrogen and hydrogen must form to achieve equilibrium" if the reactants are already favored? are we trying to make the value of Q closer to 9.60 or are we trying to make the value of K closer to 77.44? (V) In the following reaction, which of the statements is true, given theconcentrations of each species?N2(g) + 3H2 = 2NH3(g), K = 9.60[N2] = [H2] = 0.200M and [N H3] = 0.352MO The reaction is at equilibrium.equilibrium.O More nitrogen must be consumed to achieve equilibrium.cannot be established in the system.O More ammonia must form to achieveO More nitrogen and hydrogen must form to achieve equilibrium.O Equilibrium

The reaction is written as follows:N2 (g) + 3H2 (g) ⇌ 2NH3 (g)The reaction quotient for the above…

Answered: (V) In the following reaction, which of…

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

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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I don't understand this concenpt.

I know Q= 77.44 and K=9.60,

Q > K which means reactants are already favored, so why is the answer
"more nitrogen and hydrogen must form to achieve equilibrium" if the reactants are already favored?

are we trying to make the value of Q closer to 9.60 or are we trying to make the value of K closer to 77.44?

(V) In the following reaction, which of the statements is true, given the
concentrations of each species?
N2(g) + 3H2 = 2NH3(g), K = 9.60
[N2] = [H2] = 0.200M and [N H3] = 0.352M
O The reaction is at equilibrium.
equilibrium.
O More nitrogen must be consumed to achieve equilibrium.
cannot be established in the system.
O More ammonia must form to achieve
O More nitrogen and hydrogen must form to achieve equilibrium.
O Equilibrium

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