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For the reaction below, AG° = -15.0 kJ/mol at 962 K. If at 962 K, an excess of the solid A(s) is added to the gases B(g) and C(g) both having partial pressures of 0.94 atm, which statement is true? Als) 2B(g) + 2C(g) The reaction quotient will become negative. The reverse reaction will proceed spontaneously. The reaction will be at equilibrium. The equilibrium constant will increase. The forward reaction will proceed spontaneously.

For the reaction below, AG° = -15.0 kJ/mol at 962 K. If at 962 K, an excess of the solid A(s) is added to the gases B(g) and C(g) both having partial pressures of 0.94 atm, which statement is true? Als) 2B(g) + 2C(g) The reaction quotient will become negative. The reverse reaction will proceed spontaneously. The reaction will be at equilibrium. The equilibrium constant will increase. The forward reaction will proceed spontaneously.

Chemistry: The Molecular Science
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter16: Thermodynamics: Directionality Of Chemical Reactions
Section16.6: Gibbs Free Energy
Problem 16.6PSP
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For the reaction below, AG° = -15.0 kJ/mol at 962 K. If at 962 K, an excess of the solid A(s) is added to the gases B(g) and C(g) both having partial pressures of 0.94 atm, which statement is true? Als) 2B(g) + 2C(g) The reaction quotient will become negative. The reverse reaction will proceed spontaneously. The reaction will be at equilibrium. The equilibrium constant will increase. The forward reaction will proceed spontaneously.
Transcribed Image Text:For the reaction below, AG° = -15.0 kJ/mol at 962 K. If at 962 K, an excess of the solid A(s) is added to the gases B(g) and C(g) both having partial pressures of 0.94 atm, which statement is true? Als) 2B(g) + 2C(g) The reaction quotient will become negative. The reverse reaction will proceed spontaneously. The reaction will be at equilibrium. The equilibrium constant will increase. The forward reaction will proceed spontaneously.
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