6.27g of magnesium carbonate were added to an excess of sulphuric acid. The following reaction occurred:
MgCO3 + H2SO4 ---> MgSO4 +CO2 +H20
Calculate the mass of MgSO4 produced assuming a 95% yield.
Moles of MgCO3 = 0.0744
I got all the calculations correct but why is it 8.958g x 95% / 100
Doesnt make sense to me, could someone explain it please?
Turn on thread page Beta
Yield questions watch
- Thread Starter
- 02-01-2013 11:11
- 02-01-2013 11:19
So, once you have calculated the mass of MgSO4 from a perfect 100% yield (8.958), you have to take into account that the percentage yield is not 100, but 95%. Therefore, you can either multiply it by 0.95 (95% expressed as a decimal) or by 95, then divide by 100 (which is the same process, just doing it in two steps).