7. a sample of hydrogen gas is mixed with water vapor. the mix has a total pressure of 725 torr and the water vapor has a partial pressure of 24 torr. what amount (in moles) of hydrogen gas is contained in 1.85 l of this mixture at 308 k?

0.07 moles

Explanation:

According to Dalton's law, the total pressure of a mixture of gases is the sum of individual pressures exerted by the constituent gases.

Thus

Given:

Thus

According to the ideal gas equation:'

P= Pressure of the gas = 701 torr = 0.92 atm     (760torr=1atm)

V= Volume of the gas = 1.85 L

T= Temperature of the gas = 308 K

R= Value of gas constant = 0.082 Latm\K mol

Thus 0.07 moles of hydrogen gas is contained in 1.85 L of this mixture at 308 K.

the formula mass of a molecule or a compound is the sum of the atomic weights of the atoms in its empirical formula

(that's what i know about formula mass)

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