Cell Potential and Free Energy - AP Chemistry

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Question

1. $\small Zn \rightarrow $Zn^{2+}$ + $2e^{-}$$ $\small \small $E^{o}$ = 0.762 V$

2. $\small Cu \rightarrow $Cu^{2+}$ + $2e^{-}$$ $\small \small $E^{o}$= -0.340 V$

3. $\small $Zn^{2+}$ + Cu \rightarrow Zn + $Cu^{2+}$$

What is $\small \small E_${cell}^{o}$$ ? Is reaction 3 spontaneous?

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Answer

$\small $E^${o}$_{cell}$ = E_${red}^{o}$ + E_${ox}^{o}$$

$\small E_${cell}^{o}$ = -0.762 V - 0.340 V$

$\small $E^${o}$_{cell}$ = -1.1 V$

There are two concepts to consider in this problem. First, the question asks for the $\small $E^${o}$_{cell}$$ . Reaction 3 has $\small $Zn^{2+}$$ being reduced so the potential for the half reaction becomes negative. $\small Cu$ half reaction appears the same in reaction 3 so the potential is the same. Second, negative voltages indicate non-spontaneity and positive voltages are spontaneous.

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Question

1. $\small Zn \rightarrow $Zn^{2+}$ + $2e^{-}$$ $\small \small $E^{o}$ = 0.762 V$

2. $\small Cu \rightarrow $Cu^{2+}$ + $2e^{-}$$ $\small \small $E^{o}$= -0.340 V$

3. $\small $Zn^{2+}$ + Cu \rightarrow Zn + $Cu^{2+}$$

What is $\small \small E_${cell}^{o}$$ ? Is reaction 3 spontaneous?

Tap to reveal answer

Answer

$\small $E^${o}$_{cell}$ = E_${red}^{o}$ + E_${ox}^{o}$$

$\small E_${cell}^{o}$ = -0.762 V - 0.340 V$

$\small $E^${o}$_{cell}$ = -1.1 V$

There are two concepts to consider in this problem. First, the question asks for the $\small $E^${o}$_{cell}$$ . Reaction 3 has $\small $Zn^{2+}$$ being reduced so the potential for the half reaction becomes negative. $\small Cu$ half reaction appears the same in reaction 3 so the potential is the same. Second, negative voltages indicate non-spontaneity and positive voltages are spontaneous.

← Didn't Know|Knew It →

Question

1. $\small Zn \rightarrow $Zn^{2+}$ + $2e^{-}$$ $\small \small $E^{o}$ = 0.762 V$

2. $\small Cu \rightarrow $Cu^{2+}$ + $2e^{-}$$ $\small \small $E^{o}$= -0.340 V$

3. $\small $Zn^{2+}$ + Cu \rightarrow Zn + $Cu^{2+}$$

What is $\small \small E_${cell}^{o}$$ ? Is reaction 3 spontaneous?

Tap to reveal answer

Answer

$\small $E^${o}$_{cell}$ = E_${red}^{o}$ + E_${ox}^{o}$$

$\small E_${cell}^{o}$ = -0.762 V - 0.340 V$

$\small $E^${o}$_{cell}$ = -1.1 V$

There are two concepts to consider in this problem. First, the question asks for the $\small $E^${o}$_{cell}$$ . Reaction 3 has $\small $Zn^{2+}$$ being reduced so the potential for the half reaction becomes negative. $\small Cu$ half reaction appears the same in reaction 3 so the potential is the same. Second, negative voltages indicate non-spontaneity and positive voltages are spontaneous.

← Didn't Know|Knew It →

Question

1. $\small Zn \rightarrow $Zn^{2+}$ + $2e^{-}$$ $\small \small $E^{o}$ = 0.762 V$

2. $\small Cu \rightarrow $Cu^{2+}$ + $2e^{-}$$ $\small \small $E^{o}$= -0.340 V$

3. $\small $Zn^{2+}$ + Cu \rightarrow Zn + $Cu^{2+}$$

What is $\small \small E_${cell}^{o}$$ ? Is reaction 3 spontaneous?

Tap to reveal answer

Answer

$\small $E^${o}$_{cell}$ = E_${red}^{o}$ + E_${ox}^{o}$$

$\small E_${cell}^{o}$ = -0.762 V - 0.340 V$

$\small $E^${o}$_{cell}$ = -1.1 V$

There are two concepts to consider in this problem. First, the question asks for the $\small $E^${o}$_{cell}$$ . Reaction 3 has $\small $Zn^{2+}$$ being reduced so the potential for the half reaction becomes negative. $\small Cu$ half reaction appears the same in reaction 3 so the potential is the same. Second, negative voltages indicate non-spontaneity and positive voltages are spontaneous.

← Didn't Know|Knew It →

Question

1. $\small Zn \rightarrow $Zn^{2+}$ + $2e^{-}$$ $\small \small $E^{o}$ = 0.762 V$

2. $\small Cu \rightarrow $Cu^{2+}$ + $2e^{-}$$ $\small \small $E^{o}$= -0.340 V$

3. $\small $Zn^{2+}$ + Cu \rightarrow Zn + $Cu^{2+}$$

What is $\small \small E_${cell}^{o}$$ ? Is reaction 3 spontaneous?

Tap to reveal answer

Answer

$\small $E^${o}$_{cell}$ = E_${red}^{o}$ + E_${ox}^{o}$$

$\small E_${cell}^{o}$ = -0.762 V - 0.340 V$

$\small $E^${o}$_{cell}$ = -1.1 V$

There are two concepts to consider in this problem. First, the question asks for the $\small $E^${o}$_{cell}$$ . Reaction 3 has $\small $Zn^{2+}$$ being reduced so the potential for the half reaction becomes negative. $\small Cu$ half reaction appears the same in reaction 3 so the potential is the same. Second, negative voltages indicate non-spontaneity and positive voltages are spontaneous.

← Didn't Know|Knew It →

Question

1. $\small Zn \rightarrow $Zn^{2+}$ + $2e^{-}$$ $\small \small $E^{o}$ = 0.762 V$

2. $\small Cu \rightarrow $Cu^{2+}$ + $2e^{-}$$ $\small \small $E^{o}$= -0.340 V$

3. $\small $Zn^{2+}$ + Cu \rightarrow Zn + $Cu^{2+}$$

What is $\small \small E_${cell}^{o}$$ ? Is reaction 3 spontaneous?

Tap to reveal answer

Answer

$\small $E^${o}$_{cell}$ = E_${red}^{o}$ + E_${ox}^{o}$$

$\small E_${cell}^{o}$ = -0.762 V - 0.340 V$

$\small $E^${o}$_{cell}$ = -1.1 V$

There are two concepts to consider in this problem. First, the question asks for the $\small $E^${o}$_{cell}$$ . Reaction 3 has $\small $Zn^{2+}$$ being reduced so the potential for the half reaction becomes negative. $\small Cu$ half reaction appears the same in reaction 3 so the potential is the same. Second, negative voltages indicate non-spontaneity and positive voltages are spontaneous.

← Didn't Know|Knew It →

Question

1. $\small Zn \rightarrow $Zn^{2+}$ + $2e^{-}$$ $\small \small $E^{o}$ = 0.762 V$

2. $\small Cu \rightarrow $Cu^{2+}$ + $2e^{-}$$ $\small \small $E^{o}$= -0.340 V$

3. $\small $Zn^{2+}$ + Cu \rightarrow Zn + $Cu^{2+}$$

What is $\small \small E_${cell}^{o}$$ ? Is reaction 3 spontaneous?

Tap to reveal answer

Answer

$\small $E^${o}$_{cell}$ = E_${red}^{o}$ + E_${ox}^{o}$$

$\small E_${cell}^{o}$ = -0.762 V - 0.340 V$

$\small $E^${o}$_{cell}$ = -1.1 V$

There are two concepts to consider in this problem. First, the question asks for the $\small $E^${o}$_{cell}$$ . Reaction 3 has $\small $Zn^{2+}$$ being reduced so the potential for the half reaction becomes negative. $\small Cu$ half reaction appears the same in reaction 3 so the potential is the same. Second, negative voltages indicate non-spontaneity and positive voltages are spontaneous.

← Didn't Know|Knew It →

Question

1. $\small Zn \rightarrow $Zn^{2+}$ + $2e^{-}$$ $\small \small $E^{o}$ = 0.762 V$

2. $\small Cu \rightarrow $Cu^{2+}$ + $2e^{-}$$ $\small \small $E^{o}$= -0.340 V$

3. $\small $Zn^{2+}$ + Cu \rightarrow Zn + $Cu^{2+}$$

What is $\small \small E_${cell}^{o}$$ ? Is reaction 3 spontaneous?

Tap to reveal answer

Answer

$\small $E^${o}$_{cell}$ = E_${red}^{o}$ + E_${ox}^{o}$$

$\small E_${cell}^{o}$ = -0.762 V - 0.340 V$

$\small $E^${o}$_{cell}$ = -1.1 V$

There are two concepts to consider in this problem. First, the question asks for the $\small $E^${o}$_{cell}$$ . Reaction 3 has $\small $Zn^{2+}$$ being reduced so the potential for the half reaction becomes negative. $\small Cu$ half reaction appears the same in reaction 3 so the potential is the same. Second, negative voltages indicate non-spontaneity and positive voltages are spontaneous.

← Didn't Know|Knew It →

Question

1. $\small Zn \rightarrow $Zn^{2+}$ + $2e^{-}$$ $\small \small $E^{o}$ = 0.762 V$

2. $\small Cu \rightarrow $Cu^{2+}$ + $2e^{-}$$ $\small \small $E^{o}$= -0.340 V$

3. $\small $Zn^{2+}$ + Cu \rightarrow Zn + $Cu^{2+}$$

What is $\small \small E_${cell}^{o}$$ ? Is reaction 3 spontaneous?

Tap to reveal answer

Answer

$\small $E^${o}$_{cell}$ = E_${red}^{o}$ + E_${ox}^{o}$$

$\small E_${cell}^{o}$ = -0.762 V - 0.340 V$

$\small $E^${o}$_{cell}$ = -1.1 V$

There are two concepts to consider in this problem. First, the question asks for the $\small $E^${o}$_{cell}$$ . Reaction 3 has $\small $Zn^{2+}$$ being reduced so the potential for the half reaction becomes negative. $\small Cu$ half reaction appears the same in reaction 3 so the potential is the same. Second, negative voltages indicate non-spontaneity and positive voltages are spontaneous.

← Didn't Know|Knew It →

Question

1. $\small Zn \rightarrow $Zn^{2+}$ + $2e^{-}$$ $\small \small $E^{o}$ = 0.762 V$

2. $\small Cu \rightarrow $Cu^{2+}$ + $2e^{-}$$ $\small \small $E^{o}$= -0.340 V$

3. $\small $Zn^{2+}$ + Cu \rightarrow Zn + $Cu^{2+}$$

What is $\small \small E_${cell}^{o}$$ ? Is reaction 3 spontaneous?

Tap to reveal answer

Answer

$\small $E^${o}$_{cell}$ = E_${red}^{o}$ + E_${ox}^{o}$$

$\small E_${cell}^{o}$ = -0.762 V - 0.340 V$

$\small $E^${o}$_{cell}$ = -1.1 V$

There are two concepts to consider in this problem. First, the question asks for the $\small $E^${o}$_{cell}$$ . Reaction 3 has $\small $Zn^{2+}$$ being reduced so the potential for the half reaction becomes negative. $\small Cu$ half reaction appears the same in reaction 3 so the potential is the same. Second, negative voltages indicate non-spontaneity and positive voltages are spontaneous.

← Didn't Know|Knew It →

Question

1. $\small Zn \rightarrow $Zn^{2+}$ + $2e^{-}$$ $\small \small $E^{o}$ = 0.762 V$

2. $\small Cu \rightarrow $Cu^{2+}$ + $2e^{-}$$ $\small \small $E^{o}$= -0.340 V$

3. $\small $Zn^{2+}$ + Cu \rightarrow Zn + $Cu^{2+}$$

What is $\small \small E_${cell}^{o}$$ ? Is reaction 3 spontaneous?

Tap to reveal answer

Answer

$\small $E^${o}$_{cell}$ = E_${red}^{o}$ + E_${ox}^{o}$$

$\small E_${cell}^{o}$ = -0.762 V - 0.340 V$

$\small $E^${o}$_{cell}$ = -1.1 V$

There are two concepts to consider in this problem. First, the question asks for the $\small $E^${o}$_{cell}$$ . Reaction 3 has $\small $Zn^{2+}$$ being reduced so the potential for the half reaction becomes negative. $\small Cu$ half reaction appears the same in reaction 3 so the potential is the same. Second, negative voltages indicate non-spontaneity and positive voltages are spontaneous.

← Didn't Know|Knew It →

Question

1. $\small Zn \rightarrow $Zn^{2+}$ + $2e^{-}$$ $\small \small $E^{o}$ = 0.762 V$

2. $\small Cu \rightarrow $Cu^{2+}$ + $2e^{-}$$ $\small \small $E^{o}$= -0.340 V$

3. $\small $Zn^{2+}$ + Cu \rightarrow Zn + $Cu^{2+}$$

What is $\small \small E_${cell}^{o}$$ ? Is reaction 3 spontaneous?

Tap to reveal answer

Answer

$\small $E^${o}$_{cell}$ = E_${red}^{o}$ + E_${ox}^{o}$$

$\small E_${cell}^{o}$ = -0.762 V - 0.340 V$

$\small $E^${o}$_{cell}$ = -1.1 V$

There are two concepts to consider in this problem. First, the question asks for the $\small $E^${o}$_{cell}$$ . Reaction 3 has $\small $Zn^{2+}$$ being reduced so the potential for the half reaction becomes negative. $\small Cu$ half reaction appears the same in reaction 3 so the potential is the same. Second, negative voltages indicate non-spontaneity and positive voltages are spontaneous.

← Didn't Know|Knew It →

Question

1. $\small Zn \rightarrow $Zn^{2+}$ + $2e^{-}$$ $\small \small $E^{o}$ = 0.762 V$

2. $\small Cu \rightarrow $Cu^{2+}$ + $2e^{-}$$ $\small \small $E^{o}$= -0.340 V$

3. $\small $Zn^{2+}$ + Cu \rightarrow Zn + $Cu^{2+}$$

What is $\small \small E_${cell}^{o}$$ ? Is reaction 3 spontaneous?

Tap to reveal answer

Answer

$\small $E^${o}$_{cell}$ = E_${red}^{o}$ + E_${ox}^{o}$$

$\small E_${cell}^{o}$ = -0.762 V - 0.340 V$

$\small $E^${o}$_{cell}$ = -1.1 V$

There are two concepts to consider in this problem. First, the question asks for the $\small $E^${o}$_{cell}$$ . Reaction 3 has $\small $Zn^{2+}$$ being reduced so the potential for the half reaction becomes negative. $\small Cu$ half reaction appears the same in reaction 3 so the potential is the same. Second, negative voltages indicate non-spontaneity and positive voltages are spontaneous.

← Didn't Know|Knew It →

Knew It

Cell Potential and Free Energy - AP Chemistry

1. 2. 3. What is ? Is reaction 3 spontaneous?

1. 2. 3. What is ? Is reaction 3 spontaneous?

1. 2. 3. What is ? Is reaction 3 spontaneous?

1. 2. 3. What is ? Is reaction 3 spontaneous?

1. 2. 3. What is ? Is reaction 3 spontaneous?

1. 2. 3. What is ? Is reaction 3 spontaneous?

1. 2. 3. What is ? Is reaction 3 spontaneous?

1. 2. 3. What is ? Is reaction 3 spontaneous?

1. 2. 3. What is ? Is reaction 3 spontaneous?

1. 2. 3. What is ? Is reaction 3 spontaneous?

1. 2. 3. What is ? Is reaction 3 spontaneous?

1. 2. 3. What is ? Is reaction 3 spontaneous?

1. 2. 3. What is ? Is reaction 3 spontaneous?

1. $\small Zn \rightarrow $Zn^{2+}$ + $2e^{-}$$ $\small \small $E^{o}$ = 0.762 V$

2. $\small Cu \rightarrow $Cu^{2+}$ + $2e^{-}$$ $\small \small $E^{o}$= -0.340 V$

3. $\small $Zn^{2+}$ + Cu \rightarrow Zn + $Cu^{2+}$$

What is $\small \small E_${cell}^{o}$$ ? Is reaction 3 spontaneous?

1. $\small Zn \rightarrow $Zn^{2+}$ + $2e^{-}$$ $\small \small $E^{o}$ = 0.762 V$

2. $\small Cu \rightarrow $Cu^{2+}$ + $2e^{-}$$ $\small \small $E^{o}$= -0.340 V$

3. $\small $Zn^{2+}$ + Cu \rightarrow Zn + $Cu^{2+}$$

What is $\small \small E_${cell}^{o}$$ ? Is reaction 3 spontaneous?

1. $\small Zn \rightarrow $Zn^{2+}$ + $2e^{-}$$ $\small \small $E^{o}$ = 0.762 V$

2. $\small Cu \rightarrow $Cu^{2+}$ + $2e^{-}$$ $\small \small $E^{o}$= -0.340 V$

3. $\small $Zn^{2+}$ + Cu \rightarrow Zn + $Cu^{2+}$$

What is $\small \small E_${cell}^{o}$$ ? Is reaction 3 spontaneous?

1. $\small Zn \rightarrow $Zn^{2+}$ + $2e^{-}$$ $\small \small $E^{o}$ = 0.762 V$

2. $\small Cu \rightarrow $Cu^{2+}$ + $2e^{-}$$ $\small \small $E^{o}$= -0.340 V$

3. $\small $Zn^{2+}$ + Cu \rightarrow Zn + $Cu^{2+}$$

What is $\small \small E_${cell}^{o}$$ ? Is reaction 3 spontaneous?

1. $\small Zn \rightarrow $Zn^{2+}$ + $2e^{-}$$ $\small \small $E^{o}$ = 0.762 V$

2. $\small Cu \rightarrow $Cu^{2+}$ + $2e^{-}$$ $\small \small $E^{o}$= -0.340 V$

3. $\small $Zn^{2+}$ + Cu \rightarrow Zn + $Cu^{2+}$$

What is $\small \small E_${cell}^{o}$$ ? Is reaction 3 spontaneous?

1. $\small Zn \rightarrow $Zn^{2+}$ + $2e^{-}$$ $\small \small $E^{o}$ = 0.762 V$

2. $\small Cu \rightarrow $Cu^{2+}$ + $2e^{-}$$ $\small \small $E^{o}$= -0.340 V$

3. $\small $Zn^{2+}$ + Cu \rightarrow Zn + $Cu^{2+}$$

What is $\small \small E_${cell}^{o}$$ ? Is reaction 3 spontaneous?

1. $\small Zn \rightarrow $Zn^{2+}$ + $2e^{-}$$ $\small \small $E^{o}$ = 0.762 V$

2. $\small Cu \rightarrow $Cu^{2+}$ + $2e^{-}$$ $\small \small $E^{o}$= -0.340 V$

3. $\small $Zn^{2+}$ + Cu \rightarrow Zn + $Cu^{2+}$$

What is $\small \small E_${cell}^{o}$$ ? Is reaction 3 spontaneous?

1. $\small Zn \rightarrow $Zn^{2+}$ + $2e^{-}$$ $\small \small $E^{o}$ = 0.762 V$

2. $\small Cu \rightarrow $Cu^{2+}$ + $2e^{-}$$ $\small \small $E^{o}$= -0.340 V$

3. $\small $Zn^{2+}$ + Cu \rightarrow Zn + $Cu^{2+}$$

What is $\small \small E_${cell}^{o}$$ ? Is reaction 3 spontaneous?

1. $\small Zn \rightarrow $Zn^{2+}$ + $2e^{-}$$ $\small \small $E^{o}$ = 0.762 V$

2. $\small Cu \rightarrow $Cu^{2+}$ + $2e^{-}$$ $\small \small $E^{o}$= -0.340 V$

3. $\small $Zn^{2+}$ + Cu \rightarrow Zn + $Cu^{2+}$$

What is $\small \small E_${cell}^{o}$$ ? Is reaction 3 spontaneous?

1. $\small Zn \rightarrow $Zn^{2+}$ + $2e^{-}$$ $\small \small $E^{o}$ = 0.762 V$

2. $\small Cu \rightarrow $Cu^{2+}$ + $2e^{-}$$ $\small \small $E^{o}$= -0.340 V$

3. $\small $Zn^{2+}$ + Cu \rightarrow Zn + $Cu^{2+}$$

What is $\small \small E_${cell}^{o}$$ ? Is reaction 3 spontaneous?

1. $\small Zn \rightarrow $Zn^{2+}$ + $2e^{-}$$ $\small \small $E^{o}$ = 0.762 V$

2. $\small Cu \rightarrow $Cu^{2+}$ + $2e^{-}$$ $\small \small $E^{o}$= -0.340 V$

3. $\small $Zn^{2+}$ + Cu \rightarrow Zn + $Cu^{2+}$$

What is $\small \small E_${cell}^{o}$$ ? Is reaction 3 spontaneous?

1. $\small Zn \rightarrow $Zn^{2+}$ + $2e^{-}$$ $\small \small $E^{o}$ = 0.762 V$

2. $\small Cu \rightarrow $Cu^{2+}$ + $2e^{-}$$ $\small \small $E^{o}$= -0.340 V$

3. $\small $Zn^{2+}$ + Cu \rightarrow Zn + $Cu^{2+}$$

What is $\small \small E_${cell}^{o}$$ ? Is reaction 3 spontaneous?

1. $\small Zn \rightarrow $Zn^{2+}$ + $2e^{-}$$ $\small \small $E^{o}$ = 0.762 V$

2. $\small Cu \rightarrow $Cu^{2+}$ + $2e^{-}$$ $\small \small $E^{o}$= -0.340 V$

3. $\small $Zn^{2+}$ + Cu \rightarrow Zn + $Cu^{2+}$$

What is $\small \small E_${cell}^{o}$$ ? Is reaction 3 spontaneous?