What is the mass of 2n at 0.2829 atm 1.35 l and 25°c

0.437 g

From the question we have;

Pressure of the gas as 0.2829

Volume of the gas as 1.35 L

Temperature of the gas as 25°C

But, K = °C + 273.15

Therefore, temperature of the gas is equivalent to 298.15 K

We are required to calculate the mass of the gas

Using the ideal gas equation, PV = nRT , we can determine the number of moles.

R is the ideal gas constant, 0.082057 L.atm/mol.K

Therefore, rearranging the formula;

n = PV ÷ RT

 = (0.2829 atm × 1.35 L) ÷ (0.082057 × 298.15 K)

 = 0.0156 mole

Therefore, the number of moles of the gas is 0.0156 mole

We know that mass of a compound is the product of moles and the molar mass.

Mass = Moles × Molar mass

Molar mass of the gas is 28.0134 g/mol

Therefore;

         = 0.0156 mole × 28.0134 g/mol

         = 0.437 g

Thus, the mass of the gas is 0.437 g

6.4 cm (max) - 25 cm (min)

a electronegativity decreases beacuse the size of nucleus is bigger.