Determine the value of Kc for the following reaction if the equilibrium concentrations are as follows: [N2]eq = 3.6 M, [02]eq = 4.1 M, [N20]eq = 3.3 × 10-18 M. 2 N2(g) + O2(g) = 2 N?O(g) O 4.5 x 1018 O 5.0 x 5.0 × 1036 2.2 × 10-19 O2.0 × 10-37 O 4.9 × 10-17

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Determine the value of

K_{C}

for the following reaction if the equilibrium concentrations are as follows:

[N_{2}]_{eq} = 3.6 M, [O_{2}]_{eq} = 4.1 M, [N_{2} O]_{eq}

= 3.3 \times 1 0^{? 18} M

.

2 N_{2} (g) + O_{2} (g) ? 2 N_{2} O (g)

4.5 \times 1 0^{18}

5.0 \times 1 0^{36}

2.2 \times 1 0^{? 19}

2.0 \times 1 0^{? 37}

4.9 \times 1 0^{? 17}

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