Question

1. consider the flasks in the following diagram. what are the fi- nal partial pressures of h₂ and n₂ after the stopcock between the two flasks is opened? (assume the final volume is 3.00 l.) what is the total pressure (in torr)? 2.00 l h₂ 475 torr 1.00 l n₂ 0.200 atm

Explanation:

Step1: Convert pressure units

First, convert the pressure of $N_2$ from atm to torr. Since 1 atm = 760 torr, for $N_2$ with $P = 0.200$ atm, $P_{N_2 - initial}=0.200\times760 = 152$ torr.

Step2: Use Boyle's law for $H_2$

Boyle's law is $P_1V_1 = P_2V_2$. For $H_2$, $P_{1 - H_2}=475$ torr, $V_{1 - H_2}=2.00$ L and $V_{2}=3.00$ L. Then $P_{2 - H_2}=\frac{P_{1 - H_2}V_{1 - H_2}}{V_{2}}=\frac{475\times2.00}{3.00}\approx317$ torr.

Step3: Use Boyle's law for $N_2$

For $N_2$, $P_{1 - N_2}=152$ torr, $V_{1 - N_2}=1.00$ L and $V_{2}=3.00$ L. Then $P_{2 - N_2}=\frac{P_{1 - N_2}V_{1 - N_2}}{V_{2}}=\frac{152\times1.00}{3.00}\approx50.7$ torr.

Step4: Calculate total pressure

The total pressure $P_{total}=P_{2 - H_2}+P_{2 - N_2}$. So $P_{total}=317 + 50.7=368$ torr.

Answer:

The final partial - pressure of $H_2$ is approximately 317 torr, the final partial - pressure of $N_2$ is approximately 50.7 torr and the total pressure is 368 torr.