A0.455 g sample of a metal, m, reacts completely with sulfuric acid according to
m ( s ) + h 2 so 4 ( aq ) ⟶ mso 4 ( aq ) + h 2 ( g )
a volume of 207 ml of hydrogen is collected over water; the water level in the collecting vessel is the same as the outside level. atmospheric pressure is 756.0 torr, and the temperature is 25 °c. calculate the molar mass of the metal.
what is the molar mass of the metal= g/ml.

Explanation:

Several gaseous properties comprise the temperature, volume, pressure, and the number of moles of gases. These properties can be determined from each other through their relationships utilized by the ideal gas law.

Answer and Explanation:

Given:

mass of MM, m=0.502gm=0.502g

volume of hydrogen gas, V=217mL=0.217LV=217mL=0.217L

temperature, TT = 25ooC + 273.15 = 298.15K298.15K

(Using data from http://www.wiredchemist.com/chemistry/data/vapor-pressure)

vapor pressure of water at 25ooC, PwPw = 23.8torr×1atm760torr=0.0313atm23.8torr×1atm760torr=0.0313atm

total pressure, PP = 756torr×1atm760torr=0.9947atm756torr×1atm760torr=0.9947atm

universal gas constant, RR = 0.08205L⋅atmmol⋅K0.08205L⋅atmmol⋅K

The balanced chemical reaction:

MM(s) + H2SO4H2SO4(aq) ⇋⇋ MSO4MSO4(aq) + H2H2(g)

Assuming only water and hydrogen contributes to the total pressure, the partial pressure of hydrogen, PH2PH2, can be calculated from the following equation,

P=PH2+PwP=PH2+Pw

0.9947atm=PH2+0.0313atm0.9947atm=PH2+0.0313atm

PH2=0.9634atmPH2=0.9634atm

Solving for moles of H2H2, nH2nH2, using the ideal gas law,

PH2V=nH2RTPH2V=nH2RT

0.9634atm×

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