At 2000 0 C the equilibrium constant for thereaction 2NO (g) --> N 2(g) +O 2(g)

Question

At 2000 0C the equilibrium constant for thereaction 2NO(g) --> N2(g) +O2(g) is Kc= 2.4 x 103. If the intitialconcentration of NO is 0.200 M, what are the equilibrium concentrations of NO, N2, and O2 ? At 2000 0C the equilibrium constant for thereaction 2NO(g) --> N2(g) +O2(g) is Kc= 2.4 x 103. If the intitialconcentration of NO is 0.200 M, what are the equilibrium concentrations of NO, N2, and O2 ? is Kc= 2.4 x 103. If the intitialconcentration of NO is 0.200 M, what are the equilibrium concentrations of NO, N2, and O2 ?

Explanation / Answer

   2NO(g) --> N2(g) + O2(g) I   0.200 C   -2x              +x       +x E 0.200-2x         x        x Kc = [N2][O2]/[NO]2 2.4x103 = x2/ 0.200 - 2x solve for x. that will be the equilibrium concentrations of[N2] and[O2]. and [NO]= 0.200 -2x. Are you sure that the Kc value is 2.4 x 103 and not2.4 x 10-3? Hope that helps 2.4x103 = x2/ 0.200 - 2x solve for x. that will be the equilibrium concentrations of[N2] and[O2]. and [NO]= 0.200 -2x. Are you sure that the Kc value is 2.4 x 103 and not2.4 x 10-3? Hope that helps

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