What is the mass of 2N at 0.2829 atm 1.35 L and 25°C

0.437 g

Explanation:

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

Step 1: Number of moles 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

Step 2: Mass of the gas

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