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##### 2 N 2 O(g) + O 2 (g) 4 NO(g) K = [NO] 4 /[N 2 O] 2 *[O 2 ] H-(Answered)

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Question

2 N2O(g)? +? O2(g)? ? ? 4 NO(g)

K = [NO]4/[N2O]2*[O2]

H2(g)? +? CO2(g)? ? ? H2O(g)? +? CO(g)

K = [CO]*[H2O]/[CO2]*[H2]

4 HCl(g)? +? O2(g)? ? ? 2 Cl2(g)? +? 2 H2O(g)??

K = [Cl2]2*[H2O]2/[O2]*[HCl]4

3 H2(g)? +? N2(g)? ? ? 2 NH3(g)

K = [NH3]2/[N2]*[H2]3

H2(g)? +? Cl2(g)? ? ? 2HCl(g)???????

K = [HCl]2/[H2]*[Cl2]

????

2 SO2(g)? +? O2(g)? ?? 2 SO3(g)??

K = [SO3]2/[O2]*[SO2]2

Using the above equilibrium expressions, calculate the equilibrium constant, K, for the following concentrations:[N2O] = 0.0035 M, [O2] = 0.0027 M, [NO] = 5.6 x 10-9 M[H2] = 0.61 M, [CO2] = 1.6 M, [H2O] = 1.1 M, [CO] = 1.4 M[HCl] = 1.2 x 10-3 M, [O2] = 3.8 x 10-4 M, [H2O] = 5.8 x 10-2 M, [Cl2] = 5.8 x 10-2 M[NH3] = 0.62 M, [H2] = 0.14 M, [N2] = 0.45 M[H2] = 0.0045 M, [Cl2] = 0.0045 M, [HCl] = 0.0625 M[SO2] = 2.00 M, [O2] = 1.50 M, [SO3] = 3.00 M

Paper#9255925 | Written in 27-Jul-2016

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