Calculate the Kelvin temperature to which 15.0 L of a gas at 26°C would have to be heated to change the volume to 29.0 L. The pressure and number of particles remain constant.

Chemistry
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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
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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**Problem Statement:**

Calculate the Kelvin temperature to which 15.0 L of a gas at 26°C would have to be heated to change the volume to 29.0 L. The pressure and number of particles remain constant.

**Answer Box:**

\[ \square \] K

**Instructions for Solving:**

1. This problem involves the application of Charles's Law, which states that the volume of a gas is directly proportional to its temperature in Kelvin, assuming constant pressure and amount of gas.

2. The formula for Charles's Law is:

   \[
   \frac{V_1}{T_1} = \frac{V_2}{T_2}
   \]

   Where:
   - \( V_1 \) = initial volume = 15.0 L
   - \( T_1 \) = initial temperature in Kelvin
   - \( V_2 \) = final volume = 29.0 L
   - \( T_2 \) = final temperature in Kelvin

3. Convert the initial temperature from Celsius to Kelvin:

   \[
   T_1 = 26°C + 273.15 = 299.15 \, K
   \]

4. Rearrange Charles's Law to solve for \( T_2 \):

   \[
   T_2 = \frac{V_2 \cdot T_1}{V_1}
   \]

5. Perform the calculation to find \( T_2 \):

   \[
   T_2 = \frac{29.0 \, \text{L} \cdot 299.15 \, \text{K}}{15.0 \, \text{L}}
   \]

   Calculate the value to get the final Kelvin temperature.
Transcribed Image Text:**Problem Statement:** Calculate the Kelvin temperature to which 15.0 L of a gas at 26°C would have to be heated to change the volume to 29.0 L. The pressure and number of particles remain constant. **Answer Box:** \[ \square \] K **Instructions for Solving:** 1. This problem involves the application of Charles's Law, which states that the volume of a gas is directly proportional to its temperature in Kelvin, assuming constant pressure and amount of gas. 2. The formula for Charles's Law is: \[ \frac{V_1}{T_1} = \frac{V_2}{T_2} \] Where: - \( V_1 \) = initial volume = 15.0 L - \( T_1 \) = initial temperature in Kelvin - \( V_2 \) = final volume = 29.0 L - \( T_2 \) = final temperature in Kelvin 3. Convert the initial temperature from Celsius to Kelvin: \[ T_1 = 26°C + 273.15 = 299.15 \, K \] 4. Rearrange Charles's Law to solve for \( T_2 \): \[ T_2 = \frac{V_2 \cdot T_1}{V_1} \] 5. Perform the calculation to find \( T_2 \): \[ T_2 = \frac{29.0 \, \text{L} \cdot 299.15 \, \text{K}}{15.0 \, \text{L}} \] Calculate the value to get the final Kelvin temperature.
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