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Use line notation to represent each electrochemical cell in Problem 44.

a. Ni2+(aq) + Mg(s) → Ni(s) + Mg2+(aq)

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Consider the voltaic cell:

a. Determine the direction of electron flow and label the anode and the cathode.

b. Write a balanced equation for the overall reaction and calculate E°cell.

c. Label each electrode as negative or positive. 

d. Indicate the direction of anion and cation flow in the salt bridge.

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Sketch a voltaic cell for each redox reaction. Label the anode and cathode and indicate the half-reaction that occurs at each electrode and the species present in each solution. Also indicate the direction of electron flow.
c. 2 NO3 (aq) + 8 H+(aq) + 3 Cu(s) → 2 NO(g) + 4 H 2O (/) + 3 Cu2+(aq)

 

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Sketch a voltaic cell for each redox reaction. Label the anode and cathode and indicate the half-reaction that occurs at each electrode and the species present in each solution. Also indicate the direction of electron flow.
b. 2 H+(aq) + Fe(s) → H 2(g) + Fe2+(aq)

 

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Sketch a voltaic cell for each redox reaction. Label the anode and cathode and indicate the half-reaction that occurs at each electrode and the species present in each solution. Also indicate the direction of electron flow.
a. Ni2+(aq) + Mg(s) → Ni(s) + Mg2+(aq)

 

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Balance each redox reaction occurring in basic aqueous solution.
c. NO2 (aq) + Al(s) → NH3(g) + AIO2 (aq)

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Balance each redox reaction occurring in basic aqueous solution.
b. Ag(s) + CN(aq) + O2(g) → Ag(CN)2(aq)

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Balance each redox reaction occurring in basic aqueous solution.
a. MnO4(aq) + Br(aq) → MnO2(s) + BrO3(aq)

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Balance each redox reaction occurring in acidic aqueous solution.
c. NO3 (aq) + Sn2+(aq) → Sn4+(aq) + NO(g)

 

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Balance each redox reaction occurring in acidic aqueous solution.
b. ClO4(aq) + Cl(aq) → ClO3(aq) + Cl2(g)

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Balance each redox reaction occurring in acidic aqueous solution.
a. I(aq) + NO2 (aq) → I2(s) + NO(g)

 

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Balance each redox reaction occurring in acidic aqueous solution.
c. MnO4 (aq) + Al(s) → Mn 2+(aq) + Al 3+(aq)

 

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Balance each redox reaction occurring in acidic aqueous solution.
b. Mg(s) + Cr3+(aq) → Mg2+(aq) + Cr(s)

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Balance each redox reaction occurring in acidic aqueous solution.
a. Zn(s) + Sn2+(aq) → Zn2+(aq) + Sn(s)

 

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