Problem During the roasting process, how many grams of sulfur dioxide form when 10.0 mol of copper(I) sulfide reacts?Plan Referring to the balanced equation , here we are given amount of reactant (10.0 mol of Cu2S) and need the mass (g) of product (SO2) that forms. We find the amount (mol) of SO2 using the molar ratio (2 mol SO2/2 mol Cu2S) and then multiply by its molar mass (64.07 g/mol) to find the mass (g) of SO2 (see top road map).

Given: The reaction of copper (I) sulfide to give sulfur dioxide is, 2Cu2S(s) + 3O2(g)→ 2Cu2O +…

Answered: Problem During the roasting process,…

Introduction to Chemical Engineering Thermodynamics

8th Edition

ISBN:9781259696527

Author:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart

Publisher:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart

Chapter1: Introduction

Section: Chapter Questions

Problem 1.1P

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Problem During the roasting process, how many grams of sulfur dioxide form when 10.0 mol of copper(I) sulfide reacts?
Plan Referring to the balanced equation , here we are given amount of reactant (10.0 mol of Cu₂S) and need the mass (g) of product (SO₂) that forms. We find the amount (mol) of SO₂ using the molar ratio (2 mol SO₂/2 mol Cu₂S) and then multiply by its molar mass (64.07 g/mol) to find the mass (g) of SO₂ (see top road map).

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