At 35ºC, the equilibrium constant for the reaction 2NOCl(g) ![At 35ºC, the equilibrium constant for the reaction 2NOCl(g) <sub> </sub> 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<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/TB3245/11ea7cc5_01a3_6b47_a2ab_3d73afdc92bd_TB3245_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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