Convert 98.7 g Sb2S3 to mols.
Convert mols Sb2S3 to mols Sb4O6 using the coefficients in the balanced equation.
Convert mols Sb4O6 to grams Sb4O6. (This is the theoretical yield.)
Convert grams Sb4O6 to percent Sb4O6.
%Sb4O6 = [72.4/theoretical yield]*100
So basically your answer is 85.5%
86.7 kJ
<h3>
Further explanation</h3>
<u>Given:</u>
Molar mass (Mr) of ethanol = 46.07 g/mol
<u>Question:</u>
How much energy is required to vaporize 98.6 g of ethanol (C₂H₅OH) at its boiling point?
<u>The Process:</u>
Observe this . This means that 40.5 kJ of energy is required to vaporize every 1 mole of ethanol at its boiling point. Therefore we must first convert grams into moles.
<u>Question:</u>
Step-1:
Let us count the number of moles of 98.6 g of ethanol.
We obtain 2.14 moles of ethanol.
Step-2:
Let us calculate how much energy is required to vaporize 2.14 moles of ethanol at its boiling point.
The amount of energy required is
Thus, the amount of energy required to vaporize 98.6 g of ethanol at its boiling point is 86.7 kJ.
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Quick Steps
<h3>Learn more</h3>
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- Write the equilibrium constant for the reaction brainly.com/question/10608589
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Keywords: how much, energy required, to vaporize, ethanol, C₂H₅OH, its boiling point, ΔHvap, molar mass, moles, converts, kJ/mol
Answer:
C because 77.0 CsF
Explanation:
That is the correct answer because I have that homework and i got it right