The correct answer for this question is the statement 'the kinetic energy of the particles increases'. As the temperature of gas goes up, the kinetic energy of the particles increases because their velocities increase. This is because particles get excited and hit each other more - leading to increase in kinetic energy.

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spontaneous redox reaction happens between zinc (Zn) and magnesium (Mg) in an electrochemical cell. (6 points) i. Use the reduct

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Answer:

For (i): Magnesium is getting oxidized and zinc is getting reduced.

For (ii): The half reactions are given below.

For (iii): Magnesium will act as anode and zinc act as cathode.

Explanation:

For (i):

$E^o_{(Mg^{2+}/Mg)}=-2.37V\\E^o_{(Zn^{2+}/Zn)}=-0.76V$

The substance having highest positive $E^o$ potential will always get reduced and will undergo reduction reaction. Here, zinc will always undergo reduction reaction will get reduced.

Magnesium will undergo oxidation reaction and will get oxidized.

For (ii):

Oxidation reaction is defined as the reaction in which an atom looses its electrons. The oxidation number of the atom gets increased during this reaction.

$X\rightarrow X^{n+}+ne^-$

Reduction reaction is defined as the reaction in which an atom gains electrons. The oxidation number of the atom gets reduced during this reaction.

$X^{n+}+ne^-\rightarrow X$

Oxidation half reaction: $Mg\rightarrow Mg^{2+}+2e^-$

Reduction half reaction: $Zn^{2+}+2e^-\rightarrow Zn$

For (iii):

Oxidation reaction always occurs on anode side and thus, magnesium is acting as anode.

Reduction reaction always occurs on cathode side and thus, zinc is acting as cathode.

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