JEE CHEMISTRY MCQ: STATES OF MATTER

1 Medium

1 of 1

Application +4 | -1

Using van der waal's equation, calculate the constant, '

a

' (atm

\operatorname{Ltr}^2 \mathrm{~mole}^{-2}

) when two moles of a gas confined in a four litre flask exerts a pressure of

11 \mathrm{~atm}

at a temperature of

300 \mathrm{~K}

. The value of '

\mathrm{b}

' is

0.05 \mathrm{Litre}^{\text {mole }}

View answer and explanation

Correct option: A

6.5

Option A (6.5) is correct because it is the value of the van der Waals constant 'a' calculated using the given parameters in the van der Waals equation.

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A quantity of hydrogen gas occupies a volume of

30 \mathrm{~mL}

at a certain temperature and pressure. What volume would half this mass of hydrogen occupy at triple the absolute temperature and the pressure were one-ninth that of the original gas? In deriving the kinetic equation we make use of the root mean square speed of the molecules which is: Consider the following statements for kinetic molecular theory of gases
a. Particles of a gas move in all possible directions in straight lines.
b. At any particular time, different particles in the gas have different kinetic energies.
c. Collisions of gas molecules are perfectly inelastic in nature.
The correct statement(s) is/are The compressibility factor of an ideal gas is The relative strength of interionic/intermolecular forces in decreasing order is Compressibility factor of an ideal gas is