Consider the following reaction: 2 NH3(g) 2 3 H2(g) + N2(g) Kc = 2.20 1.10 mol/L of nitrogen gas, 0.50 mol/L of hydrogen gas, and 0.25 mol/L of ammonia gas are added to an empty flask. Which way, if at all, will the reaction shift to reach equilibrium? The reaction will shift left to make more reactants and reach equilibrium. The reaction is already at equilibrium and, therefore, will not shift in either direction. The reaction will shift left to make more products and reach equilibrium. The reaction will shift right to make more products and reach equilibrium. O The reaction will shift right to make more reactants and reach equilibrium.

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Chapter1: Chemical Foundations
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Consider the following reaction:
2 NH3(g) 2 3 H2(g) + N2(g)
Kc = 2.20
1.10 mol/L of nitrogen gas, 0.50 mol/L of hydrogen
gas, and 0.25 mol/L of ammonia gas are added to
an empty flask.
Which way, if at all, will the reaction shift to
reach equilibrium?
The reaction will shift left to make more
reactants and reach equilibrium.
The reaction is already at equilibrium and,
therefore, will not shift in either direction.
The reaction will shift left to make more
products and reach equilibrium.
O The reaction will shift right to make more
products and reach equilibrium.
The reaction will shift right to make more
reactants and reach equilibrium.
Transcribed Image Text:Consider the following reaction: 2 NH3(g) 2 3 H2(g) + N2(g) Kc = 2.20 1.10 mol/L of nitrogen gas, 0.50 mol/L of hydrogen gas, and 0.25 mol/L of ammonia gas are added to an empty flask. Which way, if at all, will the reaction shift to reach equilibrium? The reaction will shift left to make more reactants and reach equilibrium. The reaction is already at equilibrium and, therefore, will not shift in either direction. The reaction will shift left to make more products and reach equilibrium. O The reaction will shift right to make more products and reach equilibrium. The reaction will shift right to make more reactants and reach equilibrium.
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