
Concept explainers
Interpretation:
The amount of chlorine gas required to produce 5.00x10-3 g of chlorine mono fluoride in an excess of fluorine gas needs to be deduced based on the given reaction.
Concept Introduction:
- A
chemical reaction is represented in terms of a chemical equation with the reactants on the left and the products on the right. - The coefficient of a balanced chemical equation i.e. the stoichiometry gives the amount of reactants and products involved in the reaction.
- Chemical equations can therefore be used to determine the amount of products formed from a known quantity of reactants.

Answer to Problem 27A
Mass of Cl2 required = 3.25x10-3 g
Explanation of Solution
The given reaction is:
Step 1: Calculate the moles of ClF formed:
Mass of ClF formed = 5.00x10-3 g
Molar mass of ClF = 54.45 g/mol
Step 2: Calculate the moles of Cl2 needed:
Based on the reaction stoichiometry:
1 mole of Cl2 forms 2 mole of ClF
Therefore, 0.0918x10-3 moles of ClF will be formed upon reaction with:
Step 3: Calculate the mass of Cl2 needed:
Moles of Cl2 needed= 0.0459x10-3
Molecular weight of Cl2 = 70.9 g/mol
Therefore, mass of Cl2 required is around 3.25x10-3 g.
Chapter 9 Solutions
World of Chemistry, 3rd edition
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