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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![**Worksheet ch9b**
**Name: ___________________**
1. **What is stoichiometry?**
2. When 57.0 g copper are reacted with silver nitrate solution, Copper(II) nitrate and silver 138 g are obtained.
\_\_\_ Cu + \_\_\_ AgNO₃ → \_\_\_ Cu(NO₃)₂ + \_\_\_ Ag (unbalanced)
What is the percent yield of silver obtained?
3. Calculate the percent yield of AgBr if 375.0 g of the compound are obtained from 200.0 g of MgBr₂.
\[\text{MgBr₂ + 2 AgNO₃ → Mg(NO₃)₂ + 2 AgBr}\]
4. **Calculate number of moles in these quantities.**
a) \(5.001 \times 10^{24}\) molecules of CO₂
b) 27.18 g NaCl](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F4463fe58-173c-4775-a40a-851b460100aa%2F56955ea1-4fb1-492d-8bb8-7974f98eae2d%2Fx5godrr_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Worksheet ch9b**
**Name: ___________________**
1. **What is stoichiometry?**
2. When 57.0 g copper are reacted with silver nitrate solution, Copper(II) nitrate and silver 138 g are obtained.
\_\_\_ Cu + \_\_\_ AgNO₃ → \_\_\_ Cu(NO₃)₂ + \_\_\_ Ag (unbalanced)
What is the percent yield of silver obtained?
3. Calculate the percent yield of AgBr if 375.0 g of the compound are obtained from 200.0 g of MgBr₂.
\[\text{MgBr₂ + 2 AgNO₃ → Mg(NO₃)₂ + 2 AgBr}\]
4. **Calculate number of moles in these quantities.**
a) \(5.001 \times 10^{24}\) molecules of CO₂
b) 27.18 g NaCl
![**Worksheet ch 9a**
**Name________________________**
1. Write i) the molar mass ii) two conversion factors generated from each molar mass of the following:
a) H₂O
b) CO₂
2. Balance the chemical equation for the following:
\[
\text{C}_4\text{H}_9\text{OH} + \text{O}_2 \rightarrow \text{CO}_2 + \text{H}_2\text{O} \quad (\text{unbalanced})
\]
And set up the mole ratio of
a) O₂ to C₄H₉OH
b) CO₂ to O₂
3. How many moles of aluminum oxide will be produced from 0.50 mol of oxygen?
\[
4\text{Al} + 3 \text{O}_2 \rightarrow 2 \text{Al}_2\text{O}_3
\]
4. How many grams of CaS are produced from 2.500 moles of CaO?
\[
4 \text{HgS} + 4 \text{CaO} \rightarrow 4 \text{Hg} + 3 \text{CaS} + \text{CaSO}_4
\]
5. What mass of water is produced by the complete combustion of 225.0 g of butane?
\[
2 \text{C}_4\text{H}_{10} + 13 \text{O}_2 \rightarrow 8 \text{CO}_2 + 10 \text{H}_2\text{O}
\]
6. How many grams of CrCl₃ are required to produce 75.0 g of AgCl using the following reaction?
\[
\text{CrCl}_3 + 3 \text{AgNO}_3 \rightarrow \text{Cr(NO}_3\text{)}_3 + 3 \text{AgCl}
\]](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F4463fe58-173c-4775-a40a-851b460100aa%2F56955ea1-4fb1-492d-8bb8-7974f98eae2d%2Fhohhi38_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Worksheet ch 9a**
**Name________________________**
1. Write i) the molar mass ii) two conversion factors generated from each molar mass of the following:
a) H₂O
b) CO₂
2. Balance the chemical equation for the following:
\[
\text{C}_4\text{H}_9\text{OH} + \text{O}_2 \rightarrow \text{CO}_2 + \text{H}_2\text{O} \quad (\text{unbalanced})
\]
And set up the mole ratio of
a) O₂ to C₄H₉OH
b) CO₂ to O₂
3. How many moles of aluminum oxide will be produced from 0.50 mol of oxygen?
\[
4\text{Al} + 3 \text{O}_2 \rightarrow 2 \text{Al}_2\text{O}_3
\]
4. How many grams of CaS are produced from 2.500 moles of CaO?
\[
4 \text{HgS} + 4 \text{CaO} \rightarrow 4 \text{Hg} + 3 \text{CaS} + \text{CaSO}_4
\]
5. What mass of water is produced by the complete combustion of 225.0 g of butane?
\[
2 \text{C}_4\text{H}_{10} + 13 \text{O}_2 \rightarrow 8 \text{CO}_2 + 10 \text{H}_2\text{O}
\]
6. How many grams of CrCl₃ are required to produce 75.0 g of AgCl using the following reaction?
\[
\text{CrCl}_3 + 3 \text{AgNO}_3 \rightarrow \text{Cr(NO}_3\text{)}_3 + 3 \text{AgCl}
\]
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