Asked by Zachary Alford on May 17, 2024
Verified
What is the pressure of a gas, when it is started at 18.0 atm, 3.0 L, and 25°C, and expanded to 12.0 L and heated to 35°C?
A) 75.6 atm
B) 6.30 atm
C) 2.16 atm
D) 54.0 atm
Atm
An abbreviation for atmosphere, a unit of pressure equal to the pressure exerted by the Earth's atmosphere at sea level.
Volume
The amount of space an object or substance occupies, measured in liters, cubic meters, or other units of capacity.
°C
Degrees Celsius, a unit of temperature on the metric scale.
- Detail the interplay between temperature, pressure, volume, and the number of moles present in gases, following the ideal gas law.
Verified Answer
CS
Chelesea SawickiMay 18, 2024
Final Answer :
B
Explanation :
The pressure of the gas can be found using the combined gas law, which is P1V1/T1=P2V2/T2P_1V_1/T_1 = P_2V_2/T_2P1V1/T1=P2V2/T2 , where PPP is pressure, VVV is volume, and TTT is temperature in Kelvin. Converting the temperatures to Kelvin gives 298K (25°C + 273) and 308K (35°C + 273). Plugging in the values: 18.0 atm×3.0 L/298 K=P2×12.0 L/308 K18.0 \text{ atm} \times 3.0 \text{ L} / 298 \text{ K} = P_2 \times 12.0 \text{ L} / 308 \text{ K}18.0 atm×3.0 L/298 K=P2×12.0 L/308 K . Solving for P2P_2P2 gives approximately 6.30 atm.
Learning Objectives
- Detail the interplay between temperature, pressure, volume, and the number of moles present in gases, following the ideal gas law.