Ask Question
30 August, 07:52

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

+3
Answers (1)
  1. 30 August, 08:05
    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 the answers seem to be not correct or there’s no answer. Try a smart search to find answers to similar questions.
Search for Other Answers