A sample of nitrogen gas is collected in a 100ml container at a pressure of 688 mmhg and a temperature of 565 degrees Celsius how many grams of nitrogen gas are presented in this sample?

Mass = 36.4 ×10⁻³ g

Explanation:

Given data:

Volume of container = 100 mL ( 100/1000 = 0.1 L)

Pressure = 688 mmHg (0.9 atm)

Temperature = 565°C ( 565 + 273 = 838 K)

Mass in grams of nitrogen = ?

Solution:

According to ideal gas equation,

PV = nRT

n = number of moles

P = pressure

R = general gas constant

T = temperature

From this equation we will determine the number of moles and then we we will calculate the mass.

n = PV/RT

n = 0.9 atm × 0.1 L / 0.0821 atm. L / mol.K × 838 K

n = 0.09 / 68.8

n = 0.0013 mol

or

n = 1.3×10⁻³ mol

Mass of nitrogen gas:

Mass = number of moles × molar mass

Mass = 1.3×10⁻³ mol ×  28 g/mol

Mass = 36.4 ×10⁻³ g

the correct answer is:

a. formation of precipitation