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Statement-1. Considering van der Waals' ...

Statement-1. Considering van der Waals' equation of state of `NH_(3)` and `N_(2)`
`[P+(a)/(V^(2))][V-b] = RT`
The value of van der Waals' constant for `NH_(3)` is more than tht for `N_(2)`
Statement-2. Ammonia has lower molecular mass than `N_(2)`.

A

If both assertion and reason are correct and reason is correct explanation for assertion

B

If both assertion and reason are correct and reason is not correct explanation for assertion

C

If assertion is correct but reason is incorrect

D

If assertion and reason are both incorreect.

Text Solution

Verified by Experts

The correct Answer is:
B
Correct explanation. Ammonia is heteroatomic as well as dipolar in nature.
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Considering the van der Waals equation of state (P+a//V^(2))(V-b) =RT for ammonia (NH_(3)) and nitrogne (N_(2)) the value of a for NH_(3) is larger than that of N_(2) Ammonia has a lower molecular weight than nitrogen .

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Knowledge Check

  • STATEMENT-1: Considering the Vander Waal's equation of state (P+(a)/(V^(2)))(V-b) =RT for ammonia (NH_(3)) and nitrogen (N_(2)) . The value of a for NH_(3) is larger than that for N_(2) and STATEMENT-2: Ammonia has a lower molecular weight than nitrogen.

    A
    STATEMENT-1 is True, STATEMENT-2 is True, STATEMENT-2 is correct explanation for STATEMENT-1
    B
    STATEMENT-1 is True, STATEMENT-2 is True, STATEMENT-2 is NOT a correct explanation for STATEMENT-1
    C
    STATEMENT-1 is True, STATEMENT-2 is False
    D
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  • Statement-1. The value of van der Waals constant 'a' is higher for ammonia than for nitrogen. Statement-2 Intermoleucular hydrogen bonding is percent in ammonia.

    A
    Statement-1 is correct, Statement-2 is correct , Statement-2 is the correct explanation for Statement-1.
    B
    Statement-1 is correct, Statement-2 is correct , Statement-2 is not a correct explanation of Statement-1.
    C
    Statement-1 is correct, Statement-2 is incorrect.
    D
    Statement-1 is incorrect, Statement-2 is correct.

  • The van der Waals equation for 1 mole of gas is (p+a/V^(2))(V-b)=RT where,

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    p and V are ideal pressure and ideal volume respectively
    B
    (V - b) is the real volume
    C
    `(p+a/V^(2))` is the ideal pressure
    D
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