At 2000°C the equilibrium constant for the reaction is Kc = 2.4 103. 2 NO(g) N2(g)...
At 2000°C the equilibrium constant for the reaction is Kc = 2.4 103. 2 NO(g) N2(g) + O2(g) If the initial concentration of NO is 0.180 M, what are the equilibrium concentrations of NO, NO is not 0.002, 0.004, 0.02. 0.00180 NO is IMPORTANT, need the CORRECT answer
Homework Answers
ICE Table:
[NO]
[N2]
[O2]
initial
0.18
0
0
change -2x +1x +1x
equilibrium 0.18-2x +1x +1x
Equilibrium constant expression is
Kc = [N2]*[O2]/[NO]^2
2400.0 = (1*x)^2/(0.18-2*x)^2
sqrt(2400.0) = (1*x)/(0.18-2*x)
48.99 = (1*x)/(0.18-2*x)
8.81816-97.97959*x = 1*x
8.81816-98.97959*x = 0
x = 0.0891
At equilibrium:
[NO] = 0.180-2x = 0.180-2*0.0891 = 0.00182 M
Answer: 0.00182 M
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At 2000°C the equilibrium constant for the reaction is Kc = 2.4
103. 2 NO(g) N2(g)...
at 2000 c the equilibrium constant of the reaction is Kc = 2.4 x10 ^ 3....
at 2000 c the equilibrium constant of the reaction is
Kc = 2.4 x10 ^ 3. If the initial concentration of NO is 0.200 M.
What are the equilibrium concentrations for NO, N2 and O2
at 2000 c the equilibrium constant of the reaction is
Kc = 2.4 x10 ^ 3. If the initial concentration of NO is 0.200 M.
What are the equilibrium concentrations for NO, N2 and O2
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at 2000 c the equilibrium constant of the reaction is
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Kc = 2.4 x10 ^ 3. If the initial concentration of NO is 0.200 M.
What are the equilibrium concentrations for NO, N2 and O2
CAPÍTULO 15 Equilibrio químico A 2000 °C la constante de...
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