rEACTION YIELD QUESTION BELOW

Question

You are investigating the production of acid rain. In the lab you completed an experiment and gathered the following information:

SO3(g) + H2O(l) → H2SO4(aq)

Calculated mass of SO3 used: 40.1g

Volume of H2O used: 10mL

Concentration of the produced H2SO4: 4.9M

Volume of produced H2SO4: 20.1mL

Density of water: 1g/cm3

What is the yield of this reaction?

Answer 1

In order to find the percent yield you need to calculate how many moles of product you should have theoretically gotten given the amount of moles of reagents, and the number of moles of actual product obtained. once you know the theoretical and actual amounts, the percent yeild is a simple of ratio.

theoretical yield:

40.1 g SO3 X (1 mol SO3/80.06 g) X (1 mol H2SO4/1 mol SO3)= 0.50087 moles H2SO4

Actual Yield:

4.9 mol/L H2SO4 X (0.0201 L)= 0.09849

Percent Yield: actual/theoretical X 100

0.09849/0.50087 X 100= 19.67 % yield