Homework Help is Here – Start Your Trial Now!
Science
Chemistry
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
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
See similar textbooks
icon
Related questions
Question

Can you please answer this question and show all of the work 

### 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.
Expert Solution
trending now

Trending now

This is a popular solution!

steps

Step by step

Solved in 3 steps

SEE SOLUTIONCheck out a sample Q&A here
Blurred answer
Knowledge Booster
Quality Assurance and Calibration Methods
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.
Recommended textbooks for you
Chemistry
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Organic Chemistry
Organic Chemistry
Chemistry
ISBN:
9780078021558
Author:
Janice Gorzynski Smith Dr.
Publisher:
McGraw-Hill Education
Chemistry: Principles and Reactions
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
Elementary Principles of Chemical Processes, Bind…
Elementary Principles of Chemical Processes, Bind…
Chemistry
ISBN:
9781118431221
Author:
Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:
WILEY
SEE MORE TEXTBOOKS