Ask Question
7 November, 02:23

What is the final volume of a 400.0 mL gas sample that is subjected to a

temperature change from 22.0 °C to 30.0 °C and a pressure change from

1000 mmHg to 2 atm? (Watch your pressure!)

+5
Answers (1)
  1. 7 November, 02:38
    0
    Answer: 0.27L

    Explanation:

    Given that,

    Original volume V1 = 400.0 mL

    convert volume in milliliters to liters

    (If 1000mL = 1L

    400.0 mL = 400.0/1000 = 0.4 L)

    Original temperature T1 = 22.0 °C

    Convert temperature in Celsius to Kelvin

    (22.0 °C + 273 = 295K)

    Original pressure = 1000mmHg

    Convert pressure of 1000mmHg to atm

    (If 760mmHg = 1 atm

    1000mmHg = 1000/760 = 1.316 atm)

    New volume V2 = ?

    New Temperature T2 = 30.0°C

    (30.0°C + 273 = 303K)

    New pressure P2 = 2 atm

    Since pressure, volume and temperature are involved, apply the general gas equation

    (P1V1) T1 = (P2V2) / T2

    (1.316 atm x 0.4 L) / 295K = (2 atm x V2) / 303K

    0.526 atmL / 295K = 2V2 / 303K

    Cross multiply

    0.526 atmL x 303K = 2V2 x 295K

    159.47 = 590V2

    Divide both sides by 590

    159.47/590 = 590V2/590

    0.27 L = V2

    Thus, the final volume of the gas is 0.27L
Know the Answer?
Not Sure About the Answer?
Find an answer to your question 👍 “What is the final volume of a 400.0 mL gas sample that is subjected to a temperature change from 22.0 °C to 30.0 °C and a pressure change ...” 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