Ask Question
21 February, 09:06

A chemical reaction with an initial quantity of 1.35 moles of gas is performed in a 4.50-L flask at 24.7°C and under 1.07 atm of pressure. After the reaction is complete the final temperature is 55.2°C with a pressure of 2.92 atm. If the volume is limited by the size of the flask, how many moles of gas are present in the container after the reaction is complete?

+4
Answers (1)
  1. 21 February, 12:16
    0
    0.488 mol

    Explanation:

    By the ideal gas law:

    PV = nRT

    Where P is the pressure, V is the volume, n is the number of moles, R is the gas constant (0.082 atm. L/mol. K), and T is the temperature in K. Thus, after the reaction:

    P = 2.92 atm

    V = 4.50 L

    T = 55.2°C + 273 = 328.2 K

    PV = nRT

    n = PV/RT

    n = (2.92*4.50) / (0.082*328.2)

    n = 0.488 mol
Know the Answer?
Not Sure About the Answer?
Get an answer to your question ✅ “A chemical reaction with an initial quantity of 1.35 moles of gas is performed in a 4.50-L flask at 24.7°C and under 1.07 atm of pressure. ...” 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