Hydrogen sulfide, H,S, has the characteristic odor of rotten eggs. If a sample of HS gas at 722.6 torr and 347.8 K in a 49.9 ml. container is allowed to enter a 60.3 mL container at 464.8 K, what is the pressure in the new container? Be sure your answer has the correct number of significant figures.

Answer 1

To solve this problem, we can use the combined gas law:

P1V1/T1 = P2V2/T2

First, we need to calculate the initial pressure (P1), volume (V1), and temperature (T1) of the gas in the first container:

P1 = 722.6 torr
V1 = 49.9 mL
T1 = 347.8 K

Next, we can calculate the final pressure (P2) in the second container using the combined gas law:

P2 = (P1V1/T1) * T2/V2
P2 = (722.6 torr * 49.9 mL / 347.8 K) * 464.8 K / 60.3 mL
P2 = (36047.74 torr * K / 347.8 K) * 464.8 K / 60.3 mL
P2 = 294.46 torr

Therefore, the pressure in the new container is 294.46 torr. Rounding to three significant figures, the final answer is 294 torr.