1. Given that the equilibrium concentrations of [N2 ] = 0.035 M, [C2H2 ] = 0.057 M, and [HCN] = 6.8 × 10 -4 M, find the value of the equilibrium constant expression for the reaction N2 (g) + C2H2 (g) ⇌ 2 HCN(g)

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Chapter1: Chemical Foundations
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1. Given that the equilibrium concentrations of [N2 ] = 0.035 M, [C2H2 ] = 0.057 M, and [HCN] = 6.8 × 10 -4 M, find the value of the equilibrium constant expression for the reaction

N2 (g) + C2H2 (g) ⇌ 2 HCN(g)

2. For the above endothermic reaction, will the equilibrium reaction shift left or right or not change after the following disturbances to equilibrium. Write L, R, or U for unchanged.

addition of heat____________

addition of HCN____________

the removal of N2___________

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