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Chemistry & Chemical Reactivity

10th Edition
John C. Kotz + 3 others
ISBN: 9781337399074

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BuyFindarrow_forward

Chemistry & Chemical Reactivity

10th Edition
John C. Kotz + 3 others
ISBN: 9781337399074
Textbook Problem

Sulfuric acid can be prepared starting with the sulfide ore, cuprite (Cu2S). If each S atom in Cu2S leads to one molecule of H2SO4, what is the theoretical yield of H2SO4 from 3.00 kg of Cu2S?

Interpretation Introduction

Interpretation:

Theoretical yield of H2SO4 from 3.00kg of Cu2S has to be determined.

Concept introduction:

  Numberofmole=GivenmassofthesubstanceMolarmass

  • The molar mass of an element or compound is the mass in grams of 1 mole of that substance, and it is expressed in the unit of grams per mol (g/mol).
  • For chemical reaction balanced chemical reaction equation written in accordance with the Law of conservation of mass.
  • Law of conservation of mass states that for a reaction total mass of the reactant and product must be equal.
  • Product of a chemical reaction is the produced compounds or the compounds formed after a chemical reaction.
  • Stoichiometric factor is a relationship between reactant and product which is obtained from the balanced chemical equation for a particular reaction.
  • Theoretical yield is the maximum product yield that can be expected based on the masses of the reactants and the reaction stoichiometry.
Explanation

Here sulfuric acid is prepared from sulfide ore, cuprite (Cu2S).  Each sulfur atom in Cu2S leads to one molecule of H2SO4.  That means the stoichiometric ratio between the H2SO4 and Cu2S is 1:1

Therefore from the amount of Cu2S, mass of H2SO4 produced can be calculated as follows,

The amount (moles) of Cu2S available can be calculated by using the equation

  Numberofmole=GivenmassofthesubstanceMolarmass

  3000gCu2S×1molCu2S159.16gCu2S=18.8molCu2S

Using the stoichiometric factor calculating the amount of H2SO4 produced based on the amount of Cu2S as follows,

  18

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