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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![**Question:**
What is the mass (in grams) of 22.00 L of propane vapor (C₃H₈) at STP?
**Explanation:**
In this question, you need to determine the mass of propane gas when given its volume under standard temperature and pressure (STP) conditions.
**Key Concepts:**
- **Standard Temperature and Pressure (STP):** This refers to a temperature of 0°C (273.15 K) and a pressure of 1 atm (101.325 kPa). Under these conditions, 1 mole of an ideal gas occupies 22.4 L.
- **Molar Mass of Propane (C₃H₈):** This can be calculated by summing the atomic masses of all the atoms in a molecule of propane. Carbon (C) has an atomic mass of about 12.01 g/mol, and hydrogen (H) has an atomic mass of about 1.01 g/mol. Therefore, the molar mass of C₃H₈ is:
Molar mass = (3 × 12.01 g/mol) + (8 × 1.01 g/mol) = 44.10 g/mol.
**Calculation Steps:**
1. Determine the number of moles of propane in 22.00 L at STP using the ideal gas law concept (where 22.4 L = 1 mole at STP):
\[
\text{Moles of C₃H₈} = \frac{22.00 \, \text{L}}{22.4 \, \text{L/mol}}
\]
2. Calculate the mass using the number of moles and the molar mass of propane:
\[
\text{Mass of C₃H₈} = \text{Moles of C₃H₈} \times \text{Molar mass of C₃H₈}
\]
By following these steps, you can find the mass of 22.00 L of propane at STP.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fce0e1f50-5655-4918-bba8-458441e12ec5%2Fbc433e36-bf7a-4051-aea4-79832f8e9713%2Fvj6q1ef_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Question:**
What is the mass (in grams) of 22.00 L of propane vapor (C₃H₈) at STP?
**Explanation:**
In this question, you need to determine the mass of propane gas when given its volume under standard temperature and pressure (STP) conditions.
**Key Concepts:**
- **Standard Temperature and Pressure (STP):** This refers to a temperature of 0°C (273.15 K) and a pressure of 1 atm (101.325 kPa). Under these conditions, 1 mole of an ideal gas occupies 22.4 L.
- **Molar Mass of Propane (C₃H₈):** This can be calculated by summing the atomic masses of all the atoms in a molecule of propane. Carbon (C) has an atomic mass of about 12.01 g/mol, and hydrogen (H) has an atomic mass of about 1.01 g/mol. Therefore, the molar mass of C₃H₈ is:
Molar mass = (3 × 12.01 g/mol) + (8 × 1.01 g/mol) = 44.10 g/mol.
**Calculation Steps:**
1. Determine the number of moles of propane in 22.00 L at STP using the ideal gas law concept (where 22.4 L = 1 mole at STP):
\[
\text{Moles of C₃H₈} = \frac{22.00 \, \text{L}}{22.4 \, \text{L/mol}}
\]
2. Calculate the mass using the number of moles and the molar mass of propane:
\[
\text{Mass of C₃H₈} = \text{Moles of C₃H₈} \times \text{Molar mass of C₃H₈}
\]
By following these steps, you can find the mass of 22.00 L of propane at STP.
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