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vaieri [72.5K]
2 years ago
10

At 10.0°C and 102.5 kPa, the density of dry air is 1.26 g/L. What is the average "molar mass" of dry air at these conditions?

Chemistry
1 answer:
ivann1987 [24]2 years ago
5 0

The average "molar mass" of dry air under these conditions is 29 g/mol.

In chemistry, the molar mass of a chemical compound is described as the mass of a pattern of that compound divided by way of the amount of substance which is the number of moles in that pattern, measured in moles. The molar mass is a bulk, now not molecular, belongings of a substance.

The molar mass of a compound defines the mass of 1 mole of that unique substance and the range of grams according to the mole of a compound. In other words, the molar mass is the whole mass of all the atoms in grams that make a mole of a selected molecule. consequently, the gadgets of molar mass are grams/mole.

The ideal gas equation,

PV = nRT

number of moles = mass (m) /  Molar mass (M)

PV = m/M RT

PM = M /V RT

density = mass / volume

PM = SRT

M = SRT / P

Putting the values, M= 1.26 x 8.31 x 283k / 102.5KPa

= 28.9 g/mol

= 29 g/mol

Learn more about molar mass here brainly.com/question/21334167

#SPJ4

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