Equilibrium in thermodynamics

The video tutorial explores the relationship between the equilibrium constant (KC), Gibb's free energy (G), and the reaction quotient (QC). It explains how the sign of delta G determines the spontaneity of a reaction, with negative values indicating spontaneity and positive values indicating non-spontaneity. The tutorial also covers the thermodynamic relationship between delta G and QC, and how these relate to the equilibrium constant KC. It further discusses the conditions for spontaneity and equilibrium, and provides a case study on the formation and dissociation of nitric oxide, highlighting the implications of delta G values in these reactions.

What does a negative delta G indicate about a chemical reaction?

• The reaction is non-spontaneous and favors the backward reaction.

• The reaction is spontaneous and favors the forward reaction.

• The reaction is at equilibrium.

• The reaction has no change in free energy.

How are delta G and the reaction quotient QC related thermodynamically?

• QC is always equal to KC.

• They are related through an equation involving delta G naughty and KC.

• Delta G is always greater than QC.

• They are unrelated.

What is the equilibrium constant KC value for a spontaneous reaction?

• Equal to one

• Greater than one

• Less than one

• Zero

In the formation of nitric oxide, what does a positive delta G naughty value indicate?

• The reaction is spontaneous and favors the forward reaction.

• The reaction is non-spontaneous and favors the forward reaction.

• The reaction is non-spontaneous and favors the backward reaction.

• The reaction is at equilibrium.

What does a negative delta G naughty value indicate in the dissociation of nitric oxide?

• The reaction is non-spontaneous and favors the backward reaction.

• The reaction is spontaneous and favors the forward reaction.

• The reaction is at equilibrium.

• The reaction has no change in free energy.