A2.45 g sample of a gaseous oxide of nitrogen occupies a volume of 1.34 l at 28°c and 745 mmhg. what is the most likely formula for the gas?

The formula of nitrogen gaseous oxide is NO2.

Explanation:

Given data:

Mass of sample = 2.45 g

Volume = 1.34 L

Temperature = 28 °C                   (28+273.15 K = 301.15 k)

Pressure = 745 mmHg                (745/ 760 = 0.9803 atm)

Formula of gaseous oxide of nitrogen =?

Solution:

Gaseous oxides of nitrogen are NO, N2O , NO2 , N2O4.

Formula:

PV = nRT

n = number of moles.

n = PV / RT

n =0.9803 atm × 1.34 L / 0.0821 atm. dm³. K⁻¹ . mol⁻¹ × 301.15 K

n = 1.314 atm . L / 24.72442 atm . dm.³mol⁻¹

n = 0.05315 mol

Now we will find the number of moles in 2.45 g of sample. Gaseous oxides of nitrogen are NO, N2O , NO2 , N2O4

First of all we will solve it for N2O.

number of moles = mass / molar mass

molar mass of N2O = 44 g/mol

number of moles = 2.45 g / 44 g/mol

number of moles = 0.056 mol

Now we will solve it for NO2.

molar mass of NO2 is 46 g/mol

number of moles = 2.45 g / 46 g/mol

number of moles = 0.0533 mol

Now we will solve it for NO.

molar mass of NO is 30 g/mol.

number of moles = 2.45 g / 30 g/mol

number of moles = 0.082 mol

Now we will solve it for N2O4.

molar mass of N2O4 is 92 g/mol.

number of moles = 2.45 g / 92 g/mol

number of moles =  0.027 mol

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