Question

1. choose the the answer.

use the combined gas law to solve for the final volume.
$p_1 = 3.2$ atm
$v_1 = 2.00$ l
$t_1 = 25.0$ °c
$p_2 = 5.2$ atm
$v_2 = ?$
$t_2 = -25.0$ °c
1.02 l
1.23 l
1.48 l

Explanation:

Step1: Convert temps to Kelvin

$T_1 = 25.0 + 273.15 = 298.15\ \text{K}$
$T_2 = -25.0 + 273.15 = 248.15\ \text{K}$

Step2: State combined gas law

$$\frac{P_1V_1}{T_1} = \frac{P_2V_2}{T_2}$$

Step3: Rearrange for $V_2$

$$V_2 = \frac{P_1V_1T_2}{P_2T_1}$$

Step4: Substitute values

$$V_2 = \frac{3.2\ \text{atm} \times 2.00\ \text{L} \times 248.15\ \text{K}}{5.2\ \text{atm} \times 298.15\ \text{K}}$$

Step5: Calculate final value

$$V_2 \approx 1.02\ \text{L}$$

Answer:

1.02 L