In the manufacturing process of sulfuric acid, sulfur dioxide is reacted with oxygen to produce sulfur trioxide. using the equation, 2so2 (g) + o2 imported asset 2so3 (g), if 64.06g of sulfur dioxide is given an opportunity to react with an excess of oxygen to produce 75.00 g of sulfur trioxide, what is the percent yield of this reaction? 46.83% 60.25% 75.55% 93.68%
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Ответ:
Answer : The percent yield of the reaction is, 93.68 %
Explanation : Given,
Mass of
= 64.06 g
Molar mass of
= 64 g/mole
Molar mass of
= 80 g/mole
First we have to calculate the moles of
.
Now we have to calculate the moles of
.
The balanced chemical reaction will be,
From the balanced reaction, we conclude that
As, 2 moles of
react to give 2 moles of 
So, 1.0009 moles of
react to give 1.0009 moles of 
Now we have to calculate the mass of
The theoretical yield of
= 80.072 g
The actual yield of
= 75.00 g
Now we have to calculate the percent yield of
Therefore, the percent yield of the reaction is, 93.68 %
Ответ:
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Explanation: