A 20.00 g mixture of magnesium and zinc metal reacting with excess hydrochloric acid produced 1.042 g of hydrogen gas. What is the percent zinc in the original mixture?
A 20.00 g mixture of magnesium and zinc metal reacting with excess hydrochloric acid produced 1.042 g of hydrogen gas. What is the percent zinc in the original mixture?
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...
Related questions
Concept explainers
States of Matter
The substance that constitutes everything in the universe is known as matter. Matter comprises atoms which in turn are composed of electrons, protons, and neutrons. Different atoms combine together to give rise to molecules that act as a foundation for all kinds of substances. There are five states of matter based on their energies of attraction, namely solid, liquid, gases, plasma, and BEC (Bose-Einstein condensates).
Chemical Reactions and Equations
When a chemical species is transformed into another chemical species it is said to have undergone a chemical reaction. It consists of breaking existing bonds and forming new bonds by changing the position of electrons. These reactions are best explained using a chemical equation.
Question
100%
![**Problem Statement:**
A 20.00 g mixture of magnesium and zinc metal reacting with excess hydrochloric acid produced 1.042 g of hydrogen gas. What is the percent zinc in the original mixture?
---
**Analysis and Solution:**
To solve this problem, we need to understand the chemical reactions involved and how to use stoichiometry to find the amount of zinc in the original mixture.
### Chemical Reactions:
1. Magnesium reacts with hydrochloric acid to form magnesium chloride and hydrogen gas:
\[
\text{Mg} + 2\text{HCl} \rightarrow \text{MgCl}_2 + \text{H}_2
\]
2. Zinc reacts with hydrochloric acid to form zinc chloride and hydrogen gas:
\[
\text{Zn} + 2\text{HCl} \rightarrow \text{ZnCl}_2 + \text{H}_2
\]
### Stoichiometry:
- Molar mass of \( \text{Mg} \): 24.31 g/mol
- Molar mass of \( \text{Zn} \): 65.38 g/mol
- Molar mass of \( \text{H}_2 \): 2.02 g/mol
Given:
- Total hydrogen gas produced = 1.042 g
1. **Moles of \( \text{H}_2 \) produced:**
\[
\text{Moles of } \text{H}_2 = \frac{1.042 \, \text{g}}{2.02 \, \text{g/mol}} = 0.516 \, \text{mol}
\]
2. **Let \( x \) be the mass of magnesium and \( y \) be the mass of zinc.**
- \( x + y = 20.00 \, \text{g} \)
3. **Using stoichiometry:**
Since 1 mole of \( \text{Mg} \) or \( \text{Zn} \) produces 1 mole of \( \text{H}_2 \), use the mass ratios to solve for \( x \) and \( y \):
- The moles of Mg that could produce 0.516 mol \( \text{H}_2 \) is given by:
\[
\frac{x}{24.31 \, \](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F08752824-e903-4ce9-aeac-a3e5e1b4e67a%2F02920c77-1ebc-4ccb-bb1c-c4d546b34a7c%2Fiq2pmni_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Problem Statement:**
A 20.00 g mixture of magnesium and zinc metal reacting with excess hydrochloric acid produced 1.042 g of hydrogen gas. What is the percent zinc in the original mixture?
---
**Analysis and Solution:**
To solve this problem, we need to understand the chemical reactions involved and how to use stoichiometry to find the amount of zinc in the original mixture.
### Chemical Reactions:
1. Magnesium reacts with hydrochloric acid to form magnesium chloride and hydrogen gas:
\[
\text{Mg} + 2\text{HCl} \rightarrow \text{MgCl}_2 + \text{H}_2
\]
2. Zinc reacts with hydrochloric acid to form zinc chloride and hydrogen gas:
\[
\text{Zn} + 2\text{HCl} \rightarrow \text{ZnCl}_2 + \text{H}_2
\]
### Stoichiometry:
- Molar mass of \( \text{Mg} \): 24.31 g/mol
- Molar mass of \( \text{Zn} \): 65.38 g/mol
- Molar mass of \( \text{H}_2 \): 2.02 g/mol
Given:
- Total hydrogen gas produced = 1.042 g
1. **Moles of \( \text{H}_2 \) produced:**
\[
\text{Moles of } \text{H}_2 = \frac{1.042 \, \text{g}}{2.02 \, \text{g/mol}} = 0.516 \, \text{mol}
\]
2. **Let \( x \) be the mass of magnesium and \( y \) be the mass of zinc.**
- \( x + y = 20.00 \, \text{g} \)
3. **Using stoichiometry:**
Since 1 mole of \( \text{Mg} \) or \( \text{Zn} \) produces 1 mole of \( \text{H}_2 \), use the mass ratios to solve for \( x \) and \( y \):
- The moles of Mg that could produce 0.516 mol \( \text{H}_2 \) is given by:
\[
\frac{x}{24.31 \, \
Expert Solution
This question has been solved!
Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.
This is a popular solution!
Trending now
This is a popular solution!
Step by step
Solved in 3 steps
Knowledge Booster
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
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Organic Chemistry
Chemistry
ISBN:
9780078021558
Author:
Janice Gorzynski Smith Dr.
Publisher:
McGraw-Hill Education
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
Elementary Principles of Chemical Processes, Bind…
Chemistry
ISBN:
9781118431221
Author:
Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:
WILEY