Select the single best answer. Consider the following half-reactions: MnO4−(aq) + 8H+(aq) + 5e−→ Mn2+(aq) + 4H2O(l) NO3−(aq) + 4
1 answer:
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The balanced chemical reaction will be as follows:
To determine the % yield, first calculate the theoretical yield.
Molairty and volume of is 0.218 M and 65 mL respectively. Convert it into number of moles as follows:
Here, volume should be in L thus,
Similarly, calculate number of moles of iodide ion,
Now, from the balanced chemical equation, 1 mole of gives 1 mol of
, thus, 0.01417 mol will give 0.01417 mol of
.
Also, 2 mole of will give 1 mole of
thus, 0.0212 mol will give,
Molar mass of is 461.01 g/mol calculating mass of
obtained from
and
as follows:
From :
Similarly, for :
Here, is limiting reactant as it produced less amount of
as compared with
.
Theoretical yield is amount of product obtained from limiting reactant thus, theoretical yield will be 4.8867 g.
Percentage yield can be calculated as follows:
Actual yield is 3.26 g thus, percentage yield will be:
=66.7%
Therefore, % yield will be 66.7%