21. The product of the reaction between chromium and chlorine is chromium(III) chloride (158.35 g/mol). What mass of chlorine is required to react with excess chromium to form 79.2 g of chromium(III) chloride? 2 Cr(s) + 3 Cl2(g) → 2 CrCl3(s) а. 119 g b. 53.2 g c. 70.9 g d. 106 g
21. The product of the reaction between chromium and chlorine is chromium(III) chloride (158.35 g/mol). What mass of chlorine is required to react with excess chromium to form 79.2 g of chromium(III) chloride? 2 Cr(s) + 3 Cl2(g) → 2 CrCl3(s) а. 119 g b. 53.2 g c. 70.9 g d. 106 g
Chemistry
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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Chapter1: Chemical Foundations
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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
![**Question 21: Chemical Reaction and Stoichiometry**
In this problem, we explore the chemical reaction between chromium and chlorine, leading to the formation of chromium(III) chloride:
- **Chemical Reaction**:
\[
2 \, \text{Cr}(s) + 3 \, \text{Cl}_2(g) \rightarrow 2 \, \text{CrCl}_3(s)
\]
- **Given Data**:
- Molar mass of chromium(III) chloride (\(\text{CrCl}_3\)): 158.35 g/mol
- Mass of chromium(III) chloride to be formed: 79.2 g
The problem asks: What mass of chlorine is required to react with excess chromium to produce 79.2 g of chromium(III) chloride?
**Answer Choices**:
- a. 119 g
- b. 53.2 g (correct answer, indicated in red)
- c. 70.9 g
- d. 106 g
**Explanation**:
To solve this, you would typically:
1. Calculate the moles of \( \text{CrCl}_3 \) formed using its molar mass.
2. Use stoichiometry from the balanced equation to find the moles of \( \text{Cl}_2 \) required.
3. Convert the moles of \( \text{Cl}_2 \) to grams using its molar mass.
The correct answer is 53.2 g, as marked in red.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F4940be4b-b584-40b3-8ac6-b716dcfacd8e%2F3a9ed77e-4d10-4118-9887-c039c4dee2b8%2F2na0iir_processed.png&w=3840&q=75)
Transcribed Image Text:**Question 21: Chemical Reaction and Stoichiometry**
In this problem, we explore the chemical reaction between chromium and chlorine, leading to the formation of chromium(III) chloride:
- **Chemical Reaction**:
\[
2 \, \text{Cr}(s) + 3 \, \text{Cl}_2(g) \rightarrow 2 \, \text{CrCl}_3(s)
\]
- **Given Data**:
- Molar mass of chromium(III) chloride (\(\text{CrCl}_3\)): 158.35 g/mol
- Mass of chromium(III) chloride to be formed: 79.2 g
The problem asks: What mass of chlorine is required to react with excess chromium to produce 79.2 g of chromium(III) chloride?
**Answer Choices**:
- a. 119 g
- b. 53.2 g (correct answer, indicated in red)
- c. 70.9 g
- d. 106 g
**Explanation**:
To solve this, you would typically:
1. Calculate the moles of \( \text{CrCl}_3 \) formed using its molar mass.
2. Use stoichiometry from the balanced equation to find the moles of \( \text{Cl}_2 \) required.
3. Convert the moles of \( \text{Cl}_2 \) to grams using its molar mass.
The correct answer is 53.2 g, as marked in red.
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