Problem: At 2000°C the equilibrium constant for the reaction2NO(g) ⇌ N2(g) + O2(g)is Kc = 2.4 × 103. The initial concentration of NO is 0.200 M .a) What is the equilibrium concentration of NO? b) What is the equilibrium concentration of N2? c) What is the equilibrium concentration of O2?

Construct an ICE chart to detemrinet the equilibrium concentration.

$K_{c} = \frac{products}{reactants} = \frac{[N_{2}] [O_{2}]}{{[NO]}^{2}}$

$2.4 \times 10^{3} = \frac{(x) (x)}{0.200 - 2 x}$

$\frac{i ni t i a l [N O]}{K_{c}} = \frac{0.200}{2.4 \times 10^{3}} < < < 500; x i s r e t a i n e d i n t h e d e n o m i n a t o r$

$[2.4 \times 10^{3} = \frac{x^{2}}{0.200 - 2 x}] [0.200 - 2 x]$

$(2.4 \times 10^{3}) (0.200 - 2 x) = x^{2} 480 - 4800 x = x^{2} x^{2} + 4800 x - 480 = 0$

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At 2000°C the equilibrium constant for the reaction

2NO(g) ⇌ N₂(g) + O₂(g)

is K_c = 2.4 × 10³. The initial concentration of NO is 0.200 M .

a) What is the equilibrium concentration of NO?

b) What is the equilibrium concentration of N₂?

c) What is the equilibrium concentration of O₂?

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the ICE Chart concept. You can view video lessons to learn ICE Chart. Or if you need more ICE Chart practice, you can also practice ICE Chart practice problems.