Multiple Choice
What is the volume of total gas at STP (273.15 K and 1 atm) that is produced from the combustion of 1.00 mole of methane gas? Give your answer in liters (L).
7. Gases
The Ideal Gas Law
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A gas at 25°C and 800 torr has a volume of 105 mL. Using the Ideal Gas Law, what is the volume of the gas at standard temperature and pressure (STP)?
A
160.0 mL
B
140.0 mL
C
120.0 mL
D
87.5 mL
Verified step by step guidance1
First, understand the conditions at STP (Standard Temperature and Pressure). STP is defined as a temperature of 0°C (273.15 K) and a pressure of 1 atm (760 torr).
Convert the initial conditions to the appropriate units for the Ideal Gas Law. The initial temperature is 25°C, which needs to be converted to Kelvin: T1 = 25 + 273.15 = 298.15 K. The initial pressure is 800 torr, which can be converted to atm: P1 = 800 torr / 760 torr/atm.
Use the Ideal Gas Law in the form of the combined gas law, which relates the initial and final states of the gas: \( \frac{P_1 V_1}{T_1} = \frac{P_2 V_2}{T_2} \). Here, \( V_1 = 105 \) mL, \( P_2 = 1 \) atm, and \( T_2 = 273.15 \) K.
Rearrange the combined gas law to solve for the final volume \( V_2 \): \( V_2 = \frac{P_1 V_1 T_2}{P_2 T_1} \). Substitute the known values into this equation.
Calculate the final volume \( V_2 \) using the rearranged equation. Ensure all units are consistent and perform the arithmetic to find the volume at STP.
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