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A sample of mercury with a mass of 114.0 g was combined with 12.8 g of oxygen gas, and the resulting reaction gave 123.1 of mercury(II) oxide. How much oxygen was left over after the reaction was complete?

A sample of mercury with a mass of 114.0 g was combined with 12.8 g of oxygen gas, and the resulting reaction gave 123.1 of mercury(II) oxide. How much oxygen was left over after the reaction was complete?

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
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### Chemistry Problem: Determining Excess Reactant **Problem Statement:** A sample of mercury with a mass of 114.0 g was combined with 12.8 g of oxygen gas, and the resulting reaction gave 123.1 g of mercury(II) oxide. How much oxygen was left over after the reaction was complete? **Detailed Explanation and Solution:** To solve this problem, we need to employ the concept of conservation of mass, which states that the mass of reactants equals the mass of products in a chemical reaction. 1. **Identify the chemical equation for the reaction:** The reaction in question is the formation of mercury(II) oxide from mercury and oxygen: \( 2 \text{Hg} + \text{O}_2 \rightarrow 2 \text{HgO} \) 2. **Calculate the total mass of reactants:** - Mass of mercury (Hg): 114.0 g - Mass of oxygen (O₂): 12.8 g - Total mass of reactants: \( 114.0 \, \text{g} + 12.8 \, \text{g} = 126.8 \, \text{g} \) 3. **Compare it with the mass of products:** - Mass of mercury(II) oxide (HgO): 123.1 g 4. **Determine the mass of unreacted oxygen:** According to the conservation of mass: Mass of unreacted oxygen = Total mass of reactants - Mass of products Therefore: \( \text{Mass of unreacted oxygen} = 126.8 \, \text{g} - 123.1 \, \text{g} = 3.7 \, \text{g} \) Thus, **3.7 g of oxygen** was left over after the reaction was complete. This approach ensures that we account for the conservation of mass and accurately determine the excess reactant in the chemical reaction.
Transcribed Image Text:### Chemistry Problem: Determining Excess Reactant **Problem Statement:** A sample of mercury with a mass of 114.0 g was combined with 12.8 g of oxygen gas, and the resulting reaction gave 123.1 g of mercury(II) oxide. How much oxygen was left over after the reaction was complete? **Detailed Explanation and Solution:** To solve this problem, we need to employ the concept of conservation of mass, which states that the mass of reactants equals the mass of products in a chemical reaction. 1. **Identify the chemical equation for the reaction:** The reaction in question is the formation of mercury(II) oxide from mercury and oxygen: \( 2 \text{Hg} + \text{O}_2 \rightarrow 2 \text{HgO} \) 2. **Calculate the total mass of reactants:** - Mass of mercury (Hg): 114.0 g - Mass of oxygen (O₂): 12.8 g - Total mass of reactants: \( 114.0 \, \text{g} + 12.8 \, \text{g} = 126.8 \, \text{g} \) 3. **Compare it with the mass of products:** - Mass of mercury(II) oxide (HgO): 123.1 g 4. **Determine the mass of unreacted oxygen:** According to the conservation of mass: Mass of unreacted oxygen = Total mass of reactants - Mass of products Therefore: \( \text{Mass of unreacted oxygen} = 126.8 \, \text{g} - 123.1 \, \text{g} = 3.7 \, \text{g} \) Thus, **3.7 g of oxygen** was left over after the reaction was complete. This approach ensures that we account for the conservation of mass and accurately determine the excess reactant in the chemical reaction.
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