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a sample of gas weighs 3.33 g and occupies a volume of 1.365 l at 95 °c and 790 torr. identify the gas sample.A. Cl₂ (molar mass-70.90 g/mol)B. NH (molar mass- 17.03 g/mol)C. N₂0 molar mass-44.02 g/mol)D. CHC, (molar mass-119.4 g/mol)E. SO₂ (molar mass - 64.07 g/mol)



Answer :

tutorconsortium643

The sample of gas that will be in the container is CL2(chlorine)(molar mass= 70.90g/mol).

what is the ideal gas law?

The phrase "ideal gas" refers to a fictitious gas made up of molecules that abide by a few guidelines: Perfect gas particles do not contact or repel one another. The sole interaction between molecules of an ideal gas would be an elasticity collision when they collided or an elasticity collision with the container walls.

Briefing:

By ideal gas law, PV=nRT,

where p= pressure of the gas

V= volume occupied by the gas,

R= gas constant

T= temperature of the gas

n= no.of moles of gas

given, the mass of gas=3.33 g

           the volume of gas= 1.365ltr

          temp of gas= 95 c = 95+273.15 =368.15 k

pressure= 790 torr= 790/760= 1.03 atm

           R= 0.0820 l atm k^-1 mol ^-1

n=PV/RT

by solving, n=0.04699

MOLAR MASS= GIVEN MASS/n

so, the molar mass will come out to 70.90 g/ mol

so gas will CI2.

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