Chapter 14 IN-TEXT Example 14.4: Self-Test 14.5A

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SubparChemist
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Joined: Fri Sep 25, 2015 3:00 am

Chapter 14 IN-TEXT Example 14.4: Self-Test 14.5A

Postby SubparChemist » Mon Feb 01, 2016 3:37 pm

Brief question, for the chemical reaction formula, are we allowed to have fractions in the final equation? Or are fractions only allowed when we're trying to keep whatever we're say for example, combusting (as in last chapter), at only 1 mol?

The question states: "Write the chem. equation for the reaction corresponding to the cell Pt (s)|H2(g)|H^+(aq)||Co^3(aq), Co^2+(aq)|Pt(s)

The final answer multiplies both the reduction and oxidation reactions by two, just to eliminate the fraction in the .5H2(g)->H^+ + 1e-

For a final overall equation of H2(g) + 2Co^3+(aq) -> 2H^+(aq) + 2Co^2+(aq)

Thanks in advance

Maya Schnall 3J
Posts: 11
Joined: Fri Sep 25, 2015 3:00 am

Re: Chapter 14 IN-TEXT Example 14.4: Self-Test 14.5A

Postby Maya Schnall 3J » Mon Feb 01, 2016 7:49 pm

Although it's not technically incorrect to have fractions when balancing an equation, unless it specifically states that you're balancing for a specific number of moles of a molecule, just put integers in your final balanced equations.

Alexander Vong 3I
Posts: 56
Joined: Fri Sep 25, 2015 3:00 am

Re: Chapter 14 IN-TEXT Example 14.4: Self-Test 14.5A

Postby Alexander Vong 3I » Sat Feb 06, 2016 10:36 pm

SubparChemist wrote:
The final answer multiplies both the reduction and oxidation reactions by two, just to eliminate the fraction in the .5H2(g)->H^+ + 1e-



The half-reaction would actually be H2(g) --> 2H+(aq) + 2e-


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