A sample of gas is collected over water at a temperature of 35.0◦C when the barometric pressure reading is 642 torr. What is the partial pressure of the dry gas, given PH2O = 42.2 torr? Answer in units of torr.

The partial pressure of the dry gas is 599.8 torr

Explanation:

According to Dalton's law, the total pressure is the sum of individual pressures.

Given : =total pressure of gases = 642 torr

= partial pressure of dry gas = ?

= partial pressure of water = 42.2 torr

putting in the values we get:

Thus the partial pressure of the dry gas is 599.8 torr

b is the correct

the correct answer is option d

explanation:

i was wrong its d because they dont use cm when calculating square roots