Chapter 10: Problem 26
Under constant-pressure conditions a sample of hydrogen gas initially at \(88^{\circ} \mathrm{C}\) and \(9.6 \mathrm{~L}\) is cooled until its final volume is \(3.4 \mathrm{~L}\). What is its final temperature?
Short Answer
Expert verified
The final temperature is approximately \(-145.17 \degree C\).
Step by step solution
01
Understanding the Gas Law
The problem involves a gas undergoing a change in temperature and volume at constant pressure. This suggests the use of Charles's Law, which states that \( \frac{V_1}{T_1} = \frac{V_2}{T_2} \), where \( V \) is volume and \( T \) is temperature in Kelvin.
02
Convert Initial Temperature
Convert the initial temperature from Celsius to Kelvin. The formula for this is \( T(K) = T(\degree C) + 273.15 \). Thus, the initial temperature is \( 88 + 273.15 = 361.15 \text{ K} \).
03
Apply Charles's Law
Substitute the known values into Charles's Law: \( \frac{9.6}{361.15} = \frac{3.4}{T_2} \).
04
Solve for Final Temperature
Rearrange the equation to solve for \( T_2 \): \( T_2 = \frac{3.4 \times 361.15}{9.6} \). Calculate \( T_2 \approx 127.98 \text{ K} \).
05
Convert Final Temperature to Celsius
Convert the final temperature back to Celsius: \( T(\degree C) = T(K) - 273.15 \). Thus, \( 127.98 - 273.15 = -145.17 \degree C \).
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Key Concepts
These are the key concepts you need to understand to accurately answer the question.
constant-pressure
Charles's Law governs the behavior of gas under specific conditions. When we mention "constant-pressure," we're referring to situations where the pressure remains the same throughout the process. This constant-pressure is crucial because it allows Charles's Law to be applicable.
Charles's Law states that, at constant pressure, the volume of a gas is directly proportional to its Kelvin temperature.
This means:
Charles's Law states that, at constant pressure, the volume of a gas is directly proportional to its Kelvin temperature.
This means:
- If you increase the temperature of a gas, it expands, increasing its volume.
- Conversely, if you decrease the temperature, the gas contracts, leading to a smaller volume.
temperature conversion
Temperature conversion is a critical step when working with gas laws. Before utilizing any equations, you need to ensure the temperature is measured in Kelvin rather than Celsius.
For instance, if the initial temperature is 88°C:\[ T(K) = 88 + 273.15 = 361.15 \text{ K} \]This conversion is necessary because gas laws require temperature inputs in Kelvin to maintain proportionality and consistency in calculations.
- The Kelvin scale is an absolute scale where 0 K (Kelvin) is absolute zero, the hypothetical point where molecular motion stops.
- The Celsius scale is based on the freezing (0°C) and boiling points (100°C) of water.
For instance, if the initial temperature is 88°C:\[ T(K) = 88 + 273.15 = 361.15 \text{ K} \]This conversion is necessary because gas laws require temperature inputs in Kelvin to maintain proportionality and consistency in calculations.
gas volume change
Gas volume change under constant-pressure is directly related to changes in temperature. According to Charles's Law, when temperature decreases, the volume must also decrease proportionally, assuming constant pressure.
This relationship is described mathematically as:\[ \frac{V_1}{T_1} = \frac{V_2}{T_2} \]Where:
Calculations help us find the exact changes these variables undergo.
This relationship is described mathematically as:\[ \frac{V_1}{T_1} = \frac{V_2}{T_2} \]Where:
- \( V_1 \) and \( V_2 \) are the initial and final volumes.
- \( T_1 \) and \( T_2 \) are the initial and final temperatures in Kelvin.
Calculations help us find the exact changes these variables undergo.
Kelvin and Celsius conversion
Understanding how to interconvert Kelvin and Celsius temperatures is vital. To navigate problems involving gas laws, one must be fluent in moving between these two temperature scales.
Here's how you convert:
Here's how you convert:
- From Celsius to Kelvin: Add 273.15 to the Celsius value. For example, 88°C converts to:\[ T(K) = 88 + 273.15 = 361.15 \text{ K} \]
- From Kelvin back to Celsius: Subtract 273.15 from the Kelvin value. For instance, if an outcome gives 127.98 K, converting to Celsius yields:\[ T(\degree C) = 127.98 - 273.15 = -145.17 \degree C \]