Balance the following equations and solve the following problems using dimensional analysis. 1. Calculate the moles of solid formed from 0.652 moles HBr. FeS(s) + HBr(aq) → FeBr2(s) + H₂S(g) 2. Calculate the number of nitrogen molecules formed from 1.30 mol of NaN3. _NaN3(s)→ N2(g) + __Na(s) 3. Calculate the number of oxygen molecules needed to react with 1.00 g of manganese. Mn(s) + _O2(g) → Mn304(s)
Balance the following equations and solve the following problems using dimensional analysis. 1. Calculate the moles of solid formed from 0.652 moles HBr. FeS(s) + HBr(aq) → FeBr2(s) + H₂S(g) 2. Calculate the number of nitrogen molecules formed from 1.30 mol of NaN3. _NaN3(s)→ N2(g) + __Na(s) 3. Calculate the number of oxygen molecules needed to react with 1.00 g of manganese. Mn(s) + _O2(g) → Mn304(s)
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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![**Balancing and Problem Solving with Chemical Equations**
**Balance the following equations and solve the accompanying problems using dimensional analysis.**
1. **Calculate the moles of solid formed from 2.652 moles HBr.**
\[
\_\_ \text{FeS(s)} + \_\_ \text{HBr(aq)} \rightarrow \_\_ \text{FeBr}_2\text{(s)} + \_\_ \text{H}_2\text{S(g)}
\]
2. **Calculate the number of nitrogen molecules formed from 1.30 mol of NaN\(_3\).**
\[
\_\_ \text{NaN}_3\text{(s)} \rightarrow \_\_ \text{N}_2\text{(g)} + \_\_ \text{Na(s)}
\]
3. **Calculate the number of oxygen molecules needed to react with 1.00 g of manganese.**
\[
\_\_ \text{Mn(s)} + \_\_ \text{O}_2\text{(g)} \rightarrow \_\_ \text{Mn}_3\text{O}_4\text{(s)}
\]
**Instructions:**
- Identify and balance each chemical equation.
- Use stoichiometry to solve each problem utilizing dimensional analysis. This includes converting moles of reactants to moles of products and utilizing molar masses where necessary.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F687addeb-a453-48f6-81e2-80f2549349ce%2F8d4d9ba7-b99d-4cb7-ab9e-7b7138466d27%2Fq9jc22p_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Balancing and Problem Solving with Chemical Equations**
**Balance the following equations and solve the accompanying problems using dimensional analysis.**
1. **Calculate the moles of solid formed from 2.652 moles HBr.**
\[
\_\_ \text{FeS(s)} + \_\_ \text{HBr(aq)} \rightarrow \_\_ \text{FeBr}_2\text{(s)} + \_\_ \text{H}_2\text{S(g)}
\]
2. **Calculate the number of nitrogen molecules formed from 1.30 mol of NaN\(_3\).**
\[
\_\_ \text{NaN}_3\text{(s)} \rightarrow \_\_ \text{N}_2\text{(g)} + \_\_ \text{Na(s)}
\]
3. **Calculate the number of oxygen molecules needed to react with 1.00 g of manganese.**
\[
\_\_ \text{Mn(s)} + \_\_ \text{O}_2\text{(g)} \rightarrow \_\_ \text{Mn}_3\text{O}_4\text{(s)}
\]
**Instructions:**
- Identify and balance each chemical equation.
- Use stoichiometry to solve each problem utilizing dimensional analysis. This includes converting moles of reactants to moles of products and utilizing molar masses where necessary.
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