QuestionAll of the following statements are true EXCEPT if $\Delta G>0$ , then a reaction is not spontaneous. if $\Delta G=0$ , then $\Delta S=\Delta H$ . a reaction is spontaneous if $\Delta G<0$ . $\Delta G$ is referred to as Gibbs free energy. if $\Delta G=0$ , the system is at equilibrium.

Studdy Solution

STEP 1

1. We are given several statements about Gibbs free energy ( $\Delta G$ ).
2. We need to identify the statement that is not true.

STEP 2

1. Understand the concept of Gibbs free energy and its implications.
2. Evaluate each statement based on the understanding of Gibbs free energy.
3. Identify the incorrect statement.

STEP 3

Understand the concept of Gibbs free energy ( $\Delta G$ ): - $\Delta G$ indicates the spontaneity of a reaction. - If $\Delta G < 0$ , the reaction is spontaneous. - If $\Delta G = 0$ , the system is at equilibrium. - If $\Delta G > 0$ , the reaction is not spontaneous.

STEP 4

Evaluate the first statement: "if $\Delta G>0$ , then a reaction is not spontaneous." - This statement is true based on the understanding of Gibbs free energy.

STEP 5

Evaluate the second statement: "if $\Delta G=0$ , then $\Delta S=\Delta H$ ." - This statement is incorrect. $\Delta G = 0$ indicates equilibrium, not necessarily that $\Delta S = \Delta H$ .

STEP 6

Evaluate the third statement: "a reaction is spontaneous if $\Delta G<0$ ." - This statement is true based on the understanding of Gibbs free energy.

STEP 7

Evaluate the fourth statement: " $\Delta G$ is referred to as Gibbs free energy." - This statement is true as it is the definition of $\Delta G$ .

STEP 8

Evaluate the fifth statement: "if $\Delta G=0$ , the system is at equilibrium." - This statement is true based on the understanding of Gibbs free energy.

STEP 9

Identify the incorrect statement: - The second statement "if $\Delta G=0$ , then $\Delta S=\Delta H$ " is incorrect.
The incorrect statement is:
"if $\Delta G=0$ , then $\Delta S=\Delta H$ ."

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QuestionAll of the following statements are true EXCEPT if $\Delta G>0$ , then a reaction is not spontaneous. if $\Delta G=0$ , then $\Delta S=\Delta H$ . a reaction is spontaneous if $\Delta G<0$ . $\Delta G$ is referred to as Gibbs free energy. if $\Delta G=0$ , the system is at equilibrium.

Studdy Solution

STEP 1

1. We are given several statements about Gibbs free energy ( $\Delta G$ ).
2. We need to identify the statement that is not true.

STEP 2

1. Understand the concept of Gibbs free energy and its implications.
2. Evaluate each statement based on the understanding of Gibbs free energy.
3. Identify the incorrect statement.

STEP 3

Understand the concept of Gibbs free energy ( $\Delta G$ ): - $\Delta G$ indicates the spontaneity of a reaction. - If $\Delta G < 0$ , the reaction is spontaneous. - If $\Delta G = 0$ , the system is at equilibrium. - If $\Delta G > 0$ , the reaction is not spontaneous.

STEP 4

Evaluate the first statement: "if $\Delta G>0$ , then a reaction is not spontaneous." - This statement is true based on the understanding of Gibbs free energy.

STEP 5

Evaluate the second statement: "if $\Delta G=0$ , then $\Delta S=\Delta H$ ." - This statement is incorrect. $\Delta G = 0$ indicates equilibrium, not necessarily that $\Delta S = \Delta H$ .

STEP 6

Evaluate the third statement: "a reaction is spontaneous if $\Delta G<0$ ." - This statement is true based on the understanding of Gibbs free energy.

STEP 7

Evaluate the fourth statement: " $\Delta G$ is referred to as Gibbs free energy." - This statement is true as it is the definition of $\Delta G$ .

STEP 8

Evaluate the fifth statement: "if $\Delta G=0$ , the system is at equilibrium." - This statement is true based on the understanding of Gibbs free energy.

STEP 9

Identify the incorrect statement: - The second statement "if $\Delta G=0$ , then $\Delta S=\Delta H$ " is incorrect.
The incorrect statement is:
"if $\Delta G=0$ , then $\Delta S=\Delta H$ ."

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Studdy Solution

STEP 1

1. We are given several statements about Gibbs free energy (ΔG\Delta GΔG).2. We need to identify the statement that is not true.

STEP 2

1. Understand the concept of Gibbs free energy and its implications.2. Evaluate each statement based on the understanding of Gibbs free energy.3. Identify the incorrect statement.

STEP 3

Understand the concept of Gibbs free energy (ΔG\Delta GΔG): - ΔG\Delta GΔG indicates the spontaneity of a reaction. - If ΔG<0\Delta G < 0ΔG<0, the reaction is spontaneous. - If ΔG=0\Delta G = 0ΔG=0, the system is at equilibrium. - If ΔG>0\Delta G > 0ΔG>0, the reaction is not spontaneous.

STEP 4

Evaluate the first statement: "if ΔG>0\Delta G>0ΔG>0, then a reaction is not spontaneous." - This statement is true based on the understanding of Gibbs free energy.

STEP 5

Evaluate the second statement: "if ΔG=0\Delta G=0ΔG=0, then ΔS=ΔH\Delta S=\Delta HΔS=ΔH." - This statement is incorrect. ΔG=0\Delta G = 0ΔG=0 indicates equilibrium, not necessarily that ΔS=ΔH\Delta S = \Delta HΔS=ΔH.

STEP 6

Evaluate the third statement: "a reaction is spontaneous if ΔG<0\Delta G<0ΔG<0." - This statement is true based on the understanding of Gibbs free energy.

STEP 7

Evaluate the fourth statement: "ΔG\Delta GΔG is referred to as Gibbs free energy." - This statement is true as it is the definition of ΔG\Delta GΔG.

STEP 8

Evaluate the fifth statement: "if ΔG=0\Delta G=0ΔG=0, the system is at equilibrium." - This statement is true based on the understanding of Gibbs free energy.

STEP 9

Identify the incorrect statement: - The second statement "if ΔG=0\Delta G=0ΔG=0, then ΔS=ΔH\Delta S=\Delta HΔS=ΔH" is incorrect. The incorrect statement is:"if ΔG=0\Delta G=0ΔG=0, then ΔS=ΔH\Delta S=\Delta HΔS=ΔH."

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1. We are given several statements about Gibbs free energy ( $\Delta G$ ).
2. We need to identify the statement that is not true.

1. Understand the concept of Gibbs free energy and its implications.
2. Evaluate each statement based on the understanding of Gibbs free energy.
3. Identify the incorrect statement.

Understand the concept of Gibbs free energy ( $\Delta G$ ): - $\Delta G$ indicates the spontaneity of a reaction. - If $\Delta G < 0$ , the reaction is spontaneous. - If $\Delta G = 0$ , the system is at equilibrium. - If $\Delta G > 0$ , the reaction is not spontaneous.

Evaluate the first statement: "if $\Delta G>0$ , then a reaction is not spontaneous." - This statement is true based on the understanding of Gibbs free energy.

Evaluate the second statement: "if $\Delta G=0$ , then $\Delta S=\Delta H$ ." - This statement is incorrect. $\Delta G = 0$ indicates equilibrium, not necessarily that $\Delta S = \Delta H$ .

Evaluate the third statement: "a reaction is spontaneous if $\Delta G<0$ ." - This statement is true based on the understanding of Gibbs free energy.

Evaluate the fourth statement: " $\Delta G$ is referred to as Gibbs free energy." - This statement is true as it is the definition of $\Delta G$ .

Evaluate the fifth statement: "if $\Delta G=0$ , the system is at equilibrium." - This statement is true based on the understanding of Gibbs free energy.

Identify the incorrect statement: - The second statement "if $\Delta G=0$ , then $\Delta S=\Delta H$ " is incorrect.
The incorrect statement is:
"if $\Delta G=0$ , then $\Delta S=\Delta H$ ."