Ask Question
7 November, 13:00

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

+1
Answers (1)
  1. 7 November, 15:59
    0
    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
Know the Answer?
Not Sure About the Answer?
Find an answer to your question ✅ “What is the mass of 2N at 0.2829 atm 1.35 L and 25°C ...” in 📘 Chemistry if you're in doubt about the correctness of the answers or there's no answer, then try to use the smart search and find answers to the similar questions.
Search for Other Answers