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

Posted: Mon Feb 01, 2016 3:37 pm
by SubparChemist
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

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

Posted: Mon Feb 01, 2016 7:49 pm
by Maya Schnall 3J
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.

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

Posted: Sat Feb 06, 2016 10:36 pm
by Alexander Vong 3I
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-