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Assertion: The value of van der Waals co...

Assertion: The value of van der Waals constant a is larger for ammonia than for nitrogen.
Reason: Hydrogen bonding is present in ammonia.

A

If both (`A`) and (`R`) are correct and (`R`) is the correct explanation of (`A`).

B

If both (`A`) and (`R`) are correct, but (`R`) is not the correct explanation of (`A`).

C

If (`A`) is correct, but (`R`) is incorrect.

D

If (`A`) is incorrect, but (`R`) is correct.

Text Solution

Verified by Experts

Both assertion and reason are correct and reason is the correct explanation for assertion. The value of van der Waals constant `a` is larger for ammonia than for nitrogen.
Nitrogen is a non-polar molecule. Ammonia is a polar molecule and it shows hydrogen bonding.
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Knowledge Check

  • Assertion : The value of van der Waal's constant a is larger for ammonia than for nitrogen Reason : Hydrogen bonding is present in ammonia

    A
    Both A and R are true and R is the correct explanation of A
    B
    Both A and R are true but R is not a correct explanation of A
    C
    A is true but R is false
    D
    A is false but R is true

  • The value of van der Waals constant 'a' is makimum for

    A
    Helium
    B
    Nitrogen
    C
    `CH_(4)`
    D
    `NH_(3)`

  • The value of van der Waals constant a is the maximum for

    A
    chlorine
    B
    nitogen
    C
    Hydrogen bromide
    D
    helium

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