At 2000 K the equilibrium constant for the formation of NO (g) is 4.0 x 10-4. N2

ID: 727979 • Letter: A

Question

At 2000 K the equilibrium constant for the formation of NO (g) is 4.0 x 10-4.

N2 (g) + O2 (g) = 2 NO (g)

You have a flask in which at this temperature, the concentration of nitrogen is 0.75 mol/L, that of oxygen is 0.50 mol/L and that of NO is 4.2 x 10-3. Is the system at equilibrium and which direction will it need to proceed to reach equilibrium.

a. Yes the system is at equilibrium and a shift to the left will be observed.
b. No the system is not in equilibrium and a shift to the right will be observed.
c. No the system is not at equilibrium and a shift to the left will be observed.
d. Yes the system is at equilibrium and a shift to the right will be observed.

Explanation / Answer

(4.2 x 10-3)2/ 0.75 mol/L*0.50 mol/L =0.0004704 > K

Reaction needs to shift LEFT since Q >K

Answer is C

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At 2000 0 C the equilibrium constant for thereaction 2NO (g) --> N 2(g) +O 2(g)

At 2000 K, K_c = 0.154 for the reaction below. 2 CH_4(g) - C_2H_2(g) + 3 H_2(g)

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At 2000 K the equilibrium constant for the formation of NO (g) is 4.0 x 10-4. N2

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Explanation / Answer

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