In the reaction (SO₂ + 2H₂S → 3S + 2H₂O), 44.3g of SO₂ are mixed with 44.3g of H₂S. Calculate the maximum mass of sulfur that could be formed.

1.      Check if the equation is balanced, luckily this one is! 2.      Check if any unit conversions are needed. All masses are in grams, so no problem there. 3.      Using (moles = mass ÷ Mr), calculate: the no. of moles of SO₂ (44.3 ÷ 64.1 = 0.69); and the no. of moles of H₂S (44.3 ÷ 34.1 = 1.30). This is to work out which reagent is in excess. 4.      As there is a molar ratio of 1:2, you can divide the latter answer by 2 to get the expected no. of moles of SO₂ (0.65). Therefore, SO₂ is in excess. 5.      Use (mass = moles x Mr) to find out the mass of sulfur (0.65 x 32.1 x 3 = 62.6g). Remember to multiply by 3 to get the correct mass as you need to consider the molar ratios.

Answered by Kundai V. Chemistry tutor

3297 Views

See similar Chemistry A Level tutors

Related Chemistry A Level answers

All answers ▸

What chemical tests are appropriate to identify Butanoic acid, Propanal and 2-methyl propan-2-ol?


Pure water has a boiling point of 100 °C and a freezing point of 0 °C. What is the boiling point and freezing point of a sample of aqueous sodium chloride?


Why does silicon dioxide have a higher melting point than sulphur?


What are Van Der Waals dispersion forces?


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