Question

A 5.0L container is pressurized with 1.25 atm of hydrogen gas, 1.75 atm of oxygen, and 0.90 atm of nitrogen. What is the total pressure inside the container in atm, torr, and mmHg?

a) 3.90 atm, 2970 torr, 3960 mmHg
b) 3.90 atm, 2970 torr, 5400 mmHg
c) 4.90 atm, 2970 torr, 3960 mmHg
d) 4.90 atm, 2970 torr, 5400 mmHg

Answer 1

To find the total pressure inside the container, you add up the partial pressures of the gases present. In this case, hydrogen, oxygen, and nitrogen are present with partial pressures of 1.25 atm, 1.75 atm, and 0.90 atm, respectively. The total pressure inside the container is 4.90 atm, 3724 torr, and 3724 mmHg.

Step-by-step explanation:

To find the total pressure inside the container, you add up the partial pressures of the gases present. In this case, we have hydrogen gas with a partial pressure of 1.25 atm, oxygen with a partial pressure of 1.75 atm, and nitrogen with a partial pressure of 0.90 atm. Adding these together gives a total pressure of 4.90 atm.

To convert this to torr, which is equal to mmHg, we use the conversion factor of 1 atm = 760 torr or mmHg. So, 4.90 atm times 760 torr equals 3724 torr or mmHg.

Therefore, the total pressure inside the container is 4.90 atm, 3724 torr, and 3724 mmHg. The correct answer is option d) 4.90 atm, 2970 torr, 5400 mmHg.