Question

a gas exerts a pressure of 125.0 mm hg in a container with an unknown volume. the gas exerts a pressure of 145 mm hg when transferred to a container with a volume of 0.4650 l. what is the initial volume of the gas? v = ? l assume that the number of moles and the temperature remain constant.

Explanation:

Step1: Apply Boyle's Law

Boyle's Law: $P_1V_1 = P_2V_2$
Given: $P_1=125.0\ \text{mmHg}$, $P_2=145\ \text{mmHg}$, $V_2=0.4650\ \text{L}$
Solve for $V_1$: $V_1 = \frac{P_2V_2}{P_1}$

Step2: Calculate initial volume

Substitute values: $V_1 = \frac{145 \times 0.4650}{125.0}$
Compute: $145 \times 0.4650 = 67.425$; $\frac{67.425}{125.0} = 0.5394$

Answer:

0.5394 L