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

answer: h+ its less than oh

explanation:

1. a)c-14 has two more protons

2. d)they have different numbers of protons, neutrons, and valence electrons; they are all gases at room temperature.

3. c) iron and nickel.