Multiple Choice
At 35ºC, the equilibrium constant for the reaction 2NOCl(g) ![At 35ºC, the equilibrium constant for the reaction 2NOCl(g) 2NO(g) + Cl<sub>2</sub>(g) is K = 1.6 × 10<sup>−5</sup>.An equilibrium mixture was found to have the following concentrations of Cl<sub>2</sub> and NOCl: [Cl<sub>2</sub>] = 1.2 × 10<sup>−2</sup> M; [NOCl] = 2.8 × 10<sup>−1</sup> M.Calculate the concentration of NO(g) at equilibrium. A) 1.0 × 10<sup>−4</sup> M B) 1.0 × 10<sup>−2</sup> M C) 2.8 × 10<sup>−1</sup> M D) 2.4 × 10<sup>−2</sup> M E) 1.6 × 10<sup>−3</sup> M](https://d2lvgg3v3hfg70.cloudfront.net/TB1849/11ea78cf_0f9c_f81b_8379_d59077930e7e_TB1849_11.jpg)
2NO(g) + Cl2(g) is K = 1.6 × 10−5.An equilibrium mixture was found to have the following concentrations of Cl2 and NOCl: [Cl2] = 1.2 × 10−2 M; [NOCl] = 2.8 × 10−1 M.Calculate the concentration of NO(g) at equilibrium.
A) 1.0 × 10−4 M
B) 1.0 × 10−2 M
C) 2.8 × 10−1 M
D) 2.4 × 10−2 M
E) 1.6 × 10−3 M
Correct Answer:
Verified
Correct Answer:
Verified
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