A 56.72 g sample of nitrogen dioxide gas is sealed in a 7.55 L container and heated to a temperature of 354°C. What is the pressure of the gas?

Pressure = 27.6atm

Explanation:

Mass of nitrogen = 56.72g

Volume of the gas = 7.55L

Temperature of the gas = 354°C = (354 + 273.15)K = 627.15K

Pressure = ?

From ideal gas equation,

PV = nRT

P = pressure of the ideal gas

V = volume the gas occupies

n = number of moles of the gas

R = ideal gas constant = 0.082J/mol.K

T = temperature of the gas

Number of moles (n) = mass (m) / molar mass(M)

Molar mass of N2 = 14.0g/mol

Number of moles(n) = 56.72 / 14.0

Number of moles (n) = 4.05moles

PV = nRT

Solve for P,

P = nRT/ V

P = (4.05 × 0.082 × 627.15) / 7.55

P = 27.586atm

The pressure of the gas is approximately 27.6atm

a gas, having a molecular weight of 13 kg/kmol and a kinematic viscosity of 0.25 cm2/s, flows through a pipe 0.25 m internal diameter and 5 km long at the rate of 0.4 m3/s and is delivered at atmospheric pressure.