For the following reaction, you obtained 7.2 g of sodium sulfate, starting from 10 g of sulfuric acid. Sodium hydroxide is in excess. What is the % yield? H2SO4 + 2NaOH → Na2SO4 + 2H2O

  1. Identify the limiting reagent: you have been told sodium hydroxide is in excess, so you know sulfuric acid is the limiting reagent

  2. Calculate the moles of the limiting reagent: n = m/M. m = 10 g, M = (1 x 2) + 32.1 + (16 x 4) = 98.1 g mol-1. n = 10/98.1 = 0.10 mol

  3. The ratio of sulfuric acid to sodium sulfate is 1:1, so expected yield of sodium sulfate is 0.10 mol

  4. To work out your actual yield, calculate moles of sodium sulfate. n = m/M. m = 7.2 g, M = (23.0 x 2) + 32.1 + (16.0 x 4) = 142.1 g mol-1. n = 7.2/142.1 = 0.05 mol

  5. % yield = (actual/expected) x 100 = 50% 

RB
Answered by Rachel B. Chemistry tutor

2937 Views

See similar Chemistry A Level tutors

Related Chemistry A Level answers

All answers ▸

In the presence of ultraviolet radiation, cyclohexane reacts with bromine. A mixture of cyclic products are formed, including C6H11Br. Discuss each step of this reaction providing equations to show the mechanism.


Describe how propenal, propanal and propanone can be distinguished from one another by simple chemical tests.


What is entropy?


What type of reaction do haloalkanes undergo with nucleophiles?


We're here to help

contact us iconContact usWhatsapp logoMessage us on Whatsapptelephone icon+44 (0) 203 773 6020
Facebook logoInstagram logoLinkedIn logo

© MyTutorWeb Ltd 2013–2025

Terms & Conditions|Privacy Policy
Cookie Preferences