1. For the following reaction, the equilibrium constant Kc is 0.60 at a certain

Question

1. For the following reaction, the equilibrium constant Kc is 0.60 at a certain temperature. If the concentration of NO(g) and NOBr(g) are both 0.50 M,at equilibrium, what is the concentration of Br2(g)? 2NO(g) + Br2(g) 2NOBr(g)

a: 2.8 M

b: 1.0 M

c: 0.60 M

d: 0.36 M

e: 1.7 M

2. For the following reaction, the equilibrium concentration of NO2 is 0.38 M and equilibrium concentration of N2O4 is 1.0M. What is the value of the equilibrium constant?

2NO2(g) N2O4(g)

a: 1.0

b: 0.14

c: 2.6

d: 6.9

e: 0.38

3. 2SO2(g) + O2(g) 2SO3(g) For the reaction at equilibrium, if O2 is added, the amount of SO2 present will increase, decrease, or stay the same?

4. A solution which has [ H3O+] = 6.7 × 10-8 M is acidic, basic, or neutral?

Explanation / Answer

1. For the given reaction, 2NO(g) + Br(g) <==> 2NOBr(g)

Kc = [NOBr]^2/[NO]^2[Br2]

Feeding the given values,

[Br2] = 0.50^2/0.60 x 0.50^2 = 2.8 M

Answer : a. 2.8

2. For the given reaction,

2NO2(g) <==> N2O4(g)

Kc = [N2O4]/[NO2]^2

Feeding the given values,

Kc = 1/0.38^2 = 6.9

Answer : d. 6.9

3. According to LeChatellier's principle, when O2 is added to equilibrium mixture, the amount of SO2 would decrease as excess added O2 would react with SO2 present to form more SO3.

4. A solution with, [H3O+] = 6.7 x 10^-8 M

pH = -log[H3O+] = 7.2

The pH is slightly above 7, so the solution is mildly basic.

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