You are Here: Home

# Yield questions watch

1. 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?
2. 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).

### Related university courses

TSR Support Team

We have a brilliant team of more than 60 Support Team members looking after discussions on The Student Room, helping to make it a fun, safe and useful place to hang out.

This forum is supported by:
Updated: January 2, 2013
Today on TSR

### Summer Bucket List is Back!

Start yours and you could win £150!

### GCSE Physics Equations sheet!

Poll

The Student Room, Get Revising and Marked by Teachers are trading names of The Student Room Group Ltd.

Register Number: 04666380 (England and Wales), VAT No. 806 8067 22 Registered Office: International House, Queens Road, Brighton, BN1 3XE