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.
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.