Question

An elemental gas has a mass of 10. 3g. If the volume is 58. 4 l and the pressure is 758 torr at a tempertaure of 2. 5 c what is the gas

Answer 1

The required elemental gas which has a mass of 10.3 g in the given conditions is helium gas.

How do we calculate molar mass?

Relation between the molar mass and moles of any substance will be represented as:

n = W/M, where

• W = given mass
• M = molar mass

Moles of gas will be calculated by using the ideal gas equation:

PV = nRT, where

• P = pressure = 758 torr
• V = volume = 58.4L
• n = moles = ?
• R = universal gas constant = 62.363 L.torr / K.mol
• T = temperature = 25 degree C = 298K

On putting all values, we get moles

n = (758)(58.4) / (62.363)(298) = 44,267.2 / 18,584.2

n = 2.38 moles

Molar mass of the gas will be calculated by using the above first equation is:

M = 10.3g / 2.38mol = 4.32 g/mol = 4g/mol (approx)

Hence given elemental gas is helium.

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