Question

oth hydrogen sulfide (H2S) and ammonia (NH3) have strong, unpleasant odors. Which gas has the higher effusion rate? If you opened a container of each gas in a corner of a large room, which odor would you detect first on the other side of the room? Assume the temperature is constant. Explain your answer.

Answer 1

The molar mass of H2S is greater than the molar mass of NH3, making the velocity and effusion rate of NH3 particles faster.

Effusion rate is inversely proportional to molar mass.

NH3 will have a higher average molecule velocity, so it will diffuse faster and will reach the other side of the room more quickly.

Step-by-step explanation:

Answer 2

Answer: Odor of ammonia would we detect first on the other side of the room.

Step-by-step explanation:

To calculate the rate of diffusion of gas, we use Graham's Law.

This law states that the rate of effusion or diffusion of gas is inversely proportional to the square root of the molar mass of the gas. The equation given by this law follows:

`\text{Rate of diffusion}\propto \frac{1}{\sqrt{\text{Molar mass of the gas}}}`

`(Rate_(H_2S))/(Rate_(NH_3))=\sqrt{(M_(NH_3))/(M_(H_2S))}`

`(Rate_(H_2S))/(Rate_(NH_3))=\sqrt{(17.031)/(34.1)}`

`(Rate_(H_2S))/(Rate_(NH_3))=0.71`

Thus the odor of ammonia would we detect first on the other side of the room as the rate of effusion of ammonia would be faster as it has low molecular weight as compared to hydrogen sulphide.