
Interpretation:
The amount of sulfur that would react with 1.25 g of copper 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 number 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 22A
Mass of S = 0.630 g
Explanation of Solution
The given reaction is:
Step 1: Calculate the moles of Cu present:
Mass of Cu present = 1.25 g
The number of moles of Cu will be:
Step 2: Calculate the moles of S reacted:
Based on the reaction stoichiometry:
1 mole of Cu will react with 1 mole of S.
Therefore, 0.0197 moles of Cu will react with 0.0197 moles of S.
Step 3: Calculate the mass of S reacted:
Moles of S = 0.0197
Atomic weight of S = 32 g/mol
Mass of S will be:
Therefore, 0.630 g of S will react with 1.25 g of Cu.
Chapter 9 Solutions
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