Ask Question
21 October, 22:37

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?

+5
Answers (1)
  1. 22 October, 02:03
    0
    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
Know the Answer?
Not Sure About the Answer?
Get an answer to your question ✅ “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 ...” in 📙 Chemistry if there is no answer or all answers are wrong, use a search bar and try to find the answer among similar questions.
Search for Other Answers