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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Please show all work.
1. Find the mass of 4.52 x 10^23 particles of each of the following:
N2
Li3N
H2SO4
2. Determine the % composition of the following compounds:
MgCl2
SiO2
(NH4)2S
(also please see attachment for remaining questions and show work please)
![**Exercise 6: Determining Empirical and Molecular Formulas**
Determine the empirical and molecular formula of the following compounds:
a. **Caffeine:**
- Composition: 49.48% Carbon (C), 5.19% Hydrogen (H), 28.85% Nitrogen (N), and 16.48% Oxygen (O).
- Molar Mass: 194.2 g/mol.
- [Box for answers]
b. **Octene:**
- Composition: 85.7% Carbon (C) and 14.3% Hydrogen (H).
- Molar Mass: 112 g/mol.
- [Box for answers]
c. **An Oxide of Phosphorus:**
- Composition: 43.7% Phosphorus (P) and 56.3% Oxygen (O).
- Molar Mass: 284 g/mol.
- [Box for answers]
**Instructions:**
Calculate the empirical formula by determining the simplest whole-number ratio of moles of each element in a compound. Use the empirical formula to find the molecular formula based on the given molar mass.
**Note:**
This exercise helps reinforce understanding of concepts related to chemical composition and molecular formulas.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fec454a82-63f5-4525-9455-96f81a98ab44%2Fa7527cfc-9815-45e6-b1ea-68666b504dcc%2Fvz0e20b_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Exercise 6: Determining Empirical and Molecular Formulas**
Determine the empirical and molecular formula of the following compounds:
a. **Caffeine:**
- Composition: 49.48% Carbon (C), 5.19% Hydrogen (H), 28.85% Nitrogen (N), and 16.48% Oxygen (O).
- Molar Mass: 194.2 g/mol.
- [Box for answers]
b. **Octene:**
- Composition: 85.7% Carbon (C) and 14.3% Hydrogen (H).
- Molar Mass: 112 g/mol.
- [Box for answers]
c. **An Oxide of Phosphorus:**
- Composition: 43.7% Phosphorus (P) and 56.3% Oxygen (O).
- Molar Mass: 284 g/mol.
- [Box for answers]
**Instructions:**
Calculate the empirical formula by determining the simplest whole-number ratio of moles of each element in a compound. Use the empirical formula to find the molecular formula based on the given molar mass.
**Note:**
This exercise helps reinforce understanding of concepts related to chemical composition and molecular formulas.
Transcribed Image Text:**Chemical Reaction Problems and Calculations Guide**
**7. Oxygen Mole Calculations**
Determine the moles of \( O_2 \) that react with or are produced by 6.75 moles of the first reactant in each balanced equation:
a. \( 2C_2H_6 + 7O_2 \rightarrow 4CO_2 + 6H_2O \)
- \_\_\_\_\_
b. \( 2KClO_3 \rightarrow 2KCl + 3O_2 \)
- \_\_\_\_\_
c. \( 4Fe + 3O_2 \rightarrow 2Fe_2O_3 \)
- \_\_\_\_\_
**8. Reactant Mass Calculations**
Calculate the grams of the second reactant needed to react with 20.0 grams of the first reactant in each balanced equation:
a. \( P_4 + 6Cl_2 \rightarrow 4PCl_3 \)
- \_\_\_\_\_
b. \( P_4O_{10} + 6H_2O \rightarrow 4H_3PO_4 \)
- \_\_\_\_\_
c. \( Fe_2O_3 + 3CO \rightarrow 2Fe + 3CO_2 \)
- \_\_\_\_\_
**9. Chemical Reaction Analysis**
Using the balanced equation below, complete questions 9.a to 9.e:
\( Fe_2O_3 + 3CO \rightarrow 2Fe + 3CO_2 \)
a. Determine the grams of the first product produced from 20.0 grams of the first reactant and 20.0 grams of the second reactant.
b. Identify the limiting reactant.
c. Identify the excess reactant.
d. Calculate the grams of the reacted excess reactant.
e. Calculate the grams of the unreacted excess reactant.
**10. Reaction Yield Calculation**
Consider the reaction:
\( P_4 + 6Cl_2 \rightarrow 4PCl_3 \)
A student reacted 10.0 g of \( P_4 \) with excess \( Cl_2 \) and obtained 35.0 g of \( PCl_3 \).
a. What is the theoretical yield of \( PCl_3 \)?
- \_\_\_\_\
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