The reaction N2(g)+O2(g)⇌2NO(g) is carried out at a temperature at which Kc = 0.050. The reaction mixture starts with only the product, [NO] = 0.0300 M , and no reactants. |
Part A Find the equilibrium concentrations of N2 at equilibrium. Express your answer to two significant figures and include the appropriate units.
Part B Find the equilibrium concentrations of O2 at equilibrium. Part C Find the equilibrium concentrations of NO at equilibrium. Express your answer to two significant figures and include the appropriate units. |
Part A
Find the equilibrium concentrations of N2 at equilibrium.
Express your answer to two significant figures and include the appropriate units.
The reaction N2(g)+O2(g)⇌2NO(g) Kc = [NO]^2/[N2][O2]= 0.050 Now ICE table N2(g)+O2(g)⇌2NO(g) I 0 0 0.0300 C +x/2 +x/2 -x E x/2 x/2 0.0300-x Now kc, [NO]^2/[N2][O2]= 0.050 (0.0300-x)^2/ x/2*x/2= 0.050 X = 0.027 M |
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[N2] = X/2= 0.027/2=0.0135M |
Part B
Find the equilibrium concentrations of O2 at equilibrium.
[O2] = X/2= 0.027/2=0.0135M
Part C
Find the equilibrium concentrations of NO at equilibrium.
Express your answer to two significant figures and include the appropriate units.
[NO]= 0.0300-x = 0.0300-0.027=0.003M
Cross check
Now kc,
[NO]^2/[N2][O2]= 0.050
= (0.003)^2/0.0135*0.0135
=0.050
The reaction N2(g)+O2(g)⇌2NO(g) is carried out at a temperature at which Kc = 0.050. The reaction mixture...
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