Multiple Choice
What is the density of ammonia gas (NH3) at a pressure of 2.00 atm and a temperature of 25.0°C, assuming ideal gas behavior?
7. Gases
The Ideal Gas Law Applications
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Using the Ideal Gas Law, calculate the final temperature when 2.00 L of an ideal gas at 20.0°C is compressed to 1.00 L, assuming constant pressure.
A
5.0°C
B
0.0°C
C
10.0°C
D
15.0°C
Verified step by step guidance1
Start by recalling the Ideal Gas Law, which is expressed as \( PV = nRT \), where \( P \) is pressure, \( V \) is volume, \( n \) is the number of moles, \( R \) is the ideal gas constant, and \( T \) is temperature in Kelvin.
Since the problem states that the pressure is constant and the number of moles of gas does not change, we can use the combined gas law: \( \frac{V_1}{T_1} = \frac{V_2}{T_2} \). This equation relates the initial and final states of the gas.
Convert the initial temperature from Celsius to Kelvin by adding 273.15. So, \( T_1 = 20.0 + 273.15 \) K.
Substitute the known values into the combined gas law equation: \( \frac{2.00}{T_1} = \frac{1.00}{T_2} \).
Solve for \( T_2 \) by rearranging the equation: \( T_2 = \frac{1.00 \times T_1}{2.00} \). Calculate \( T_2 \) in Kelvin and then convert it back to Celsius by subtracting 273.15.
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