1. Determine empirical formula and molecular formula for the compound that is 25.5% carbon, 6.38% hydrogen, and 68.1% sulfur. Its molecular mass is close to 100 grams.
1. Determine empirical formula and molecular formula for the compound that is 25.5% carbon, 6.38% hydrogen, and 68.1% sulfur. Its molecular mass is close to 100 grams.
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...
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![### Chemistry Problem Set
#### 1. Empirical and Molecular Formulas
Determine the empirical formula and molecular formula for a compound composed of 25.5% carbon, 6.38% hydrogen, and 68.1% sulfur. The molecular mass is close to 100 grams.
#### 2. Mass Percent Composition
Calculate the mass percent composition of the elements in \( \text{Mg(NO}_3\text{)}_2 \).
- \( \% \text{Mg} = \_\_\_\_\_\_ \)
- \( \% \text{N} = \_\_\_\_\_\_ \)
- \( \% \text{O} = \_\_\_\_\_\_ \)
#### 3. Water Production Calculation
Determine the grams of \( \text{H}_2\text{O} \) produced if you start with 33.2 g of \( \text{Mg(OH)}_2 \).
Reaction:
\[ \text{Mg(OH)}_2 + 2 \text{HCl} \rightarrow \text{MgCl}_2 + 2 \text{H}_2\text{O} \]
- \( 33.2 \, \text{g} \rightarrow \, \text{g} \)
#### 4. Limiting Reagent and Excess Reactant Analysis
For the reaction quantities shown below, identify the limiting reagent and excess reactant. Calculate the grams of \( \text{TiO}_2 \) produced and the grams of excess reactant not consumed.
Reaction:
\[ \text{TiCl}_4 + 2 \text{H}_2\text{O} \rightarrow \text{TiO}_2 + 4 \text{HCl} \]
Given:
- \( 7.14 \, \text{g TiCl}_4 \)
- \( 2.12 \, \text{g H}_2\text{O} \)
Calculate:
- \( \, \text{g TiO}_2 \)
- \( \, \text{g}\) of excess reactant not consumed.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F7cb7ab84-2909-44b4-aa38-afda86b9d9a5%2F12176331-9736-43e7-91e4-99dca6f28d5a%2F0sgbrq9_processed.png&w=3840&q=75)
Transcribed Image Text:### Chemistry Problem Set
#### 1. Empirical and Molecular Formulas
Determine the empirical formula and molecular formula for a compound composed of 25.5% carbon, 6.38% hydrogen, and 68.1% sulfur. The molecular mass is close to 100 grams.
#### 2. Mass Percent Composition
Calculate the mass percent composition of the elements in \( \text{Mg(NO}_3\text{)}_2 \).
- \( \% \text{Mg} = \_\_\_\_\_\_ \)
- \( \% \text{N} = \_\_\_\_\_\_ \)
- \( \% \text{O} = \_\_\_\_\_\_ \)
#### 3. Water Production Calculation
Determine the grams of \( \text{H}_2\text{O} \) produced if you start with 33.2 g of \( \text{Mg(OH)}_2 \).
Reaction:
\[ \text{Mg(OH)}_2 + 2 \text{HCl} \rightarrow \text{MgCl}_2 + 2 \text{H}_2\text{O} \]
- \( 33.2 \, \text{g} \rightarrow \, \text{g} \)
#### 4. Limiting Reagent and Excess Reactant Analysis
For the reaction quantities shown below, identify the limiting reagent and excess reactant. Calculate the grams of \( \text{TiO}_2 \) produced and the grams of excess reactant not consumed.
Reaction:
\[ \text{TiCl}_4 + 2 \text{H}_2\text{O} \rightarrow \text{TiO}_2 + 4 \text{HCl} \]
Given:
- \( 7.14 \, \text{g TiCl}_4 \)
- \( 2.12 \, \text{g H}_2\text{O} \)
Calculate:
- \( \, \text{g TiO}_2 \)
- \( \, \text{g}\) of excess reactant not consumed.
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