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Chapter 6: Problem 89

Balance each of the following oxidation-reduction reactions by using the oxidation states method. a. \(\mathrm{C}_{2} \mathrm{H}_{6}(g)+\mathrm{O}_{2}(g) \rightarrow \mathrm{CO}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(g)\) b. \(\mathrm{Mg}(s)+\mathrm{HCl}(a q) \rightarrow \mathrm{Mg}^{2+}(a q)+\mathrm{Cl}^{-}(a q)+\mathrm{H}_{2}(g)\) c. \(\mathrm{Co}^{3+}(a q)+\mathrm{Ni}(s) \rightarrow \mathrm{Co}^{2+}(a q)+\mathrm{Ni}^{2+}(a q)\) d. \(\mathrm{Zn}(s)+\mathrm{H}_{2} \mathrm{SO}_{4}(a q) \rightarrow \mathrm{ZnSO}_{4}(a q)+\mathrm{H}_{2}(g)\)

Short Answer

Expert verified
The balanced reactions are: a. \[\mathrm{C}_{2}\mathrm{H}_{6}(g) + \frac{7}{2}\mathrm{O}_{2}(g) \rightarrow 2\mathrm{CO}_{2}(g) + 3\mathrm{H}_{2}\mathrm{O}(g)\] b. \[\mathrm{Mg}(s) + 2\mathrm{HCl}(a q) \rightarrow \mathrm{Mg}^{2+}(a q) + 2\mathrm{Cl}^{-}(a q) + \mathrm{H}_{2}(g)\] c. \[2\mathrm{Co}^{3+}(a q) + 2\mathrm{Ni}(s) \rightarrow 2\mathrm{Co}^{2+}(a q) + 2\mathrm{Ni}^{2+}(a q)\] d. \[\mathrm{Zn}(s) + \mathrm{H}_{2}\mathrm{SO}_{4}(a q) \rightarrow \mathrm{ZnSO}_{4}(a q) + \mathrm{H}_{2}(g)\]

Step by step solution

01

1. Identify oxidation and reduction processes

In this reaction, carbon in \(\mathrm{C}_{2}\mathrm{H}_{6}\) gets oxidized to carbon dioxide \(\mathrm{CO}_{2}\), and oxygen in \(\mathrm{O}_{2}\) gets reduced to water \(\mathrm{H}_{2}\mathrm{O}\).
02

2. Determine the oxidation states of elements

The oxidation state of hydrogen is +1, carbon in ethane is -3, carbon in carbon dioxide is +4, and oxygen in oxygen gas and water is -2.
03

3. Balance the electrons gained and lost

Carbon goes from -3 to +4, losing 7 electrons in the process. Oxygen goes from 0 to -2, gaining 2 electrons. To balance the electrons, we need 2 carbon atoms and 7 oxygen atoms.
04

4. Balance the elements and overall reaction

The balanced reaction is: \[\mathrm{C}_{2}\mathrm{H}_{6}(g) + \frac{7}{2}\mathrm{O}_{2}(g) \rightarrow 2\mathrm{CO}_{2}(g) + 3\mathrm{H}_{2}\mathrm{O}(g)\] #b. Balancing \(\mathrm{Mg}(s)+\mathrm{HCl}(a q) \rightarrow \mathrm{Mg}^{2+}(a q)+\mathrm{Cl}^{-}(a q)+\mathrm{H}_{2}(g)\)#
05

1. Identify oxidation and reduction processes

In this reaction, magnesium is oxidized to \(\mathrm{Mg}^{2+}\) and hydrogen in \(\mathrm{HCl}\) is reduced to \(\mathrm{H}_{2}\).
06

2. Determine the oxidation states of elements

The oxidation state of magnesium is 0, magnesium in \(\mathrm{Mg}^{2+}\) is +2, hydrogen in \(\mathrm{HCl}\) is +1, and hydrogen in \(\mathrm{H}_{2}\) is 0.
07

3. Balance the electrons gained and lost

Magnesium goes from 0 to +2, losing 2 electrons. Hydrogen goes from +1 to 0, gaining 1 electron. To balance the electrons, we need 2 hydrogen atoms.
08

4. Balance the elements and overall reaction

The balanced reaction is: \[\mathrm{Mg}(s) + 2\mathrm{HCl}(a q) \rightarrow \mathrm{Mg}^{2+}(a q) + 2\mathrm{Cl}^{-}(a q) + \mathrm{H}_{2}(g)\] #c. Balancing \(\mathrm{Co}^{3+}(a q)+\mathrm{Ni}(s) \rightarrow \mathrm{Co}^{2+}(a q)+\mathrm{Ni}^{2+}(a q)\)#
09

1. Identify oxidation and reduction processes

In this reaction, nickel gets oxidized to \(\mathrm{Ni}^{2+}\), and cobalt in \(\mathrm{Co}^{3+}\) gets reduced to \(\mathrm{Co}^{2+}\).
10

2. Determine the oxidation states of elements

The oxidation state of nickel is 0, nickel in \(\mathrm{Ni}^{2+}\) is +2, cobalt in \(\mathrm{Co}^{3+}\) is +3, and cobalt in \(\mathrm{Co}^{2+}\) is +2.
11

3. Balance the electrons gained and lost

Nickel goes from 0 to +2, losing 2 electrons. Cobalt goes from +3 to +2, gaining 1 electron. To balance the electrons, we need 2 cobalt atoms.
12

4. Balance the elements and overall reaction

The balanced reaction is: \[2\mathrm{Co}^{3+}(a q) + 2\mathrm{Ni}(s) \rightarrow 2\mathrm{Co}^{2+}(a q) + 2\mathrm{Ni}^{2+}(a q)\] #d. Balancing \(\mathrm{Zn}(s)+\mathrm{H}_{2} \mathrm{SO}_{4}(a q) \rightarrow \mathrm{ZnSO}_{4}(a q)+\mathrm{H}_{2}(g)\)#
13

1. Identify oxidation and reduction processes

In this reaction, zinc gets oxidized to \(\mathrm{ZnSO}_{4}\) and hydrogen in \(\mathrm{H}_{2}\mathrm{SO}_{4}\) gets reduced to \(\mathrm{H}_{2}\).
14

2. Determine the oxidation states of elements

The oxidation state of zinc is 0, zinc in \(\mathrm{ZnSO}_{4}\) is +2, hydrogen in \(\mathrm{H}_{2}\mathrm{SO}_{4}\) is +1, and hydrogen in \(\mathrm{H}_{2}\) is 0.
15

3. Balance the electrons gained and lost

Zinc goes from 0 to +2, losing 2 electrons. Hydrogen goes from +1 to 0, gaining 1 electron. To balance the electrons, we need 2 hydrogen atoms.
16

4. Balance the elements and overall reaction

The balanced reaction is: \[\mathrm{Zn}(s) + \mathrm{H}_{2}\mathrm{SO}_{4}(a q) \rightarrow \mathrm{ZnSO}_{4}(a q) + \mathrm{H}_{2}(g)\]

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