ChemistryThe pressure exerted by 2.0 mol of a van der Waal gas (a = 366 k Pa dm6mol–2 and b = 0.05 dm3mol–1) at T= 300 K and V=12.1dm3 is (use R = 8.32 kPa dm3 K–1 mol–1)

The pressure exerted by 2.0 mol of a van der Waal gas (a = 366 k Pa dm6mol–2 and b = 0.05 dm3mol–1) at T= 300 K and V=12.1dm3 is (use R = 8.32 kPa dm3 K–1 mol–1)

  1. A

    395.0kPa

  2. B

    406.0kPa

  3. C

    420.1kPa

  4. D

    435.6kPa

    Fill Out the Form for Expert Academic Guidance!l



    +91



    Live ClassesBooksTest SeriesSelf Learning



    Verify OTP Code (required)

    I agree to the terms and conditions and privacy policy.

    Solution:

    The van der waals equation of state is: P+an2V2V-nb=nRT P+366 kPa dm6mol-2×2212.1 dm312.1 dm3-2×0.05 dm3mol-1 =2×8.32 kPa dm3K-1mol-1×300 P=406.0 kPa

    Chat on WhatsApp Call Infinity Learn

      Talk to our academic expert!



      +91


      Live ClassesBooksTest SeriesSelf Learning




      Verify OTP Code (required)

      I agree to the terms and conditions and privacy policy.