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<sub>c</sub> = 1.6×10<sup>-5</sup>.An equilibrium mixture was found to have the following concentrations of Cl<sup>2</sup> 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/TB6485/11eab46b_9caf_0eb1_a889_e5c94b3a1bc5_TB6485_11.jpg)
2NO(g) + Cl2(g) is Kc = 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
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