If under a given set of conditions the reaction A → B occurs with ΔG = -14 kJ/mol, and the reaction C→ B occurs with ΔG =- 16 kJ/mol, then: a. Conversion of A to C is exergonic. b. A and C can never be at equilibrium, even under different reaction conditions. c. Oconversion of A to C is entropically driven. d. Conversion of C to A is freely reversible.

a. Conversion of A to C is exergonic.

Explanation:

In the problem:  C→ B occurs with ΔG = + 16 kJ/mol

It is possible to sum ΔG of reactions to obtain ΔG of another related reaction:

A → B ΔG = -14kJ/mol

C → B ΔG = +16kJ/mol

A → C ΔG = -14kJ/mol - (+16kJ/mol) = -30kJ/mol

As ΔG < 0

The reaction is exergonic

Under these condition, the reaction occurs. But under another conditions, the reaction will be at equilibrium (ΔG = 0)

A reaction is entropically driven if ΔG < 0 and ΔS is high. But we don't have information of ΔS.

As ΔG <0, the reaction is not spontaneous in the reverse direction

Right option is:

answer: c. the experiment shows that the red substance experienced a chemical change.

explanation: chemical change is the change in which chemical composition of the substance changes. physical change is the change in which there is no change in chemical composition.

chemical changes are accompanied by following changes:

a) precipitate formation

b) energy is released or absorbed

c) formation of bubbles

d) change in color

as it is given that the red color has disappeared and there is production of gas, it means the red substance has undergone a chemical change.

e

the atomic mass is the bottom number on the element.

-steel jelly