A fixed quantity of gas has a pressure of 1.35 atm, a volume of 23.8 L, and a temperature of 205.1 K. If the pressure increases to 2.84 atm and the temperature rises to 233.4 K, what is the new volume of the gas?
A) 0.183 L
B) 7.06 L
C) 9.94 L
D) 12.9 L
E) 57.0 L

Question

Quizplus · Accepted Answer

The initial state of the gas can be described by the equation:
P1V1/T1 = nR
where P1 = 1.35 atm, V1 = 23.8 L, and T1 = 205.1 K.
The final state of the gas can be described by the equation:
P2V2/T2 = nR
where P2 = 2.84 atm, T2 = 233.4 K, and V2 is the unknown.
Since the amount of gas (n) and the gas constant (R) are constant, we can set the two equations equal to each other and solve for V2:
P1V1/T1 = P2V2/T2
V2 = (P1/T1) * (T2/P2) * V1
Plugging in the given values, we get:
V2 = (1.35 atm/205.1 K) * (233.4 K/2.84 atm) * 23.8 L
V2 ≈ 12.9 L

A Fixed Quantity of Gas Has a Pressure of 1