Ask Question
2 February, 20:29

If a sample of H2 has a volume of 22.4 L at 273.0 K and 760.0 mmHg, what will the volume be if the pressure decreases to 650.0 mmHg and the temperature increases to 320.0K?

+5
Answers (2)
  1. 2 February, 21:38
    0
    the serious answer:

    final volume or V2 = 30.7 liters

    Explanation:

    Considering that the values that this problem gives you are: the value of V1 or initial volume of the gas, T1 and T2 which are initial and final temperature, and as for the pressure it gives you P1 and P2, that is, the values also of initial pressure and finally.

    So up to here we have all the values, except for the final volume, that is, when that gas changed its temperature and pressure ... what V2 or volume did it reach?

    That is why we will use the following equation:

    P1 x V1 / T1 = p2 x v2 / T2

    We clear V2 from this equation, so as the final equation we would have:

    V2 = (760X22,4X320) / (273X650) = 30.7 liters
  2. 2 February, 22:19
    0
    30.7L

    Explanation:

    The following data were obtained from the question:

    V1 (initial volume) = 22.4L

    T1 (initial temperature) = 273K

    P1 (initial pressure) = 760mmHg

    P2 (final pressure) = 650mmHg

    T2 (final temperature) = 320K

    V2 (final volume) = ?

    Using the general gas equation P1V1/T1 = P2V2/T2, the final volume of the gas can be obtained as follow:

    P1V1/T1 = P2V2/T2

    760x22.4/273 = 650xV2/320

    Cross multiply to express in linear form

    273 x 650 x V2 = 760 x 22.4 x 320

    Divide both side by 273 x 650

    V2 = (760 x 22.4 x 320) / (273 x 650)

    V2 = 30.7L

    Therefore, the new volume of the gas will be 30.7L
Know the Answer?
Not Sure About the Answer?
Find an answer to your question ✅ “If a sample of H2 has a volume of 22.4 L at 273.0 K and 760.0 mmHg, what will the volume be if the pressure decreases to 650.0 mmHg and the ...” 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