Mock Test 1 — States of Matter

The volume of $0.1$ mol of a gas at $25°$C and $1$ atm:

Two gases A and B effuse through same orifice. Ratio of rates: $r_A/r_B = 2$. Ratio of $M_A/M_B$:

At very high pressures, the compressibility factor of a real gas:

The molar volume of a gas at NTP ($20°$C, $1$ atm):

Order of RMS speed at same temperature: $H_2$, $N_2$, $O_2$, $CO_2$:

Boyle's law graph: $P$ vs $1/V$ at const T is:

The vapour pressure of a liquid at $373$ K equals atmospheric pressure of $1$ atm. This means:

In van der Waals equation, $a$ corrects for:

Hydrogen bond is strongest in:

Surface tension of water at room temperature:

Volume of $4$ g of CH₄ at STP (in L):

Compressibility factor at ideal behavior:

Number of H-bonds each water molecule can form (max):

Assertion (A): Boiling point of water is higher than that of H₂S. Reason (R): Water has hydrogen bonding while H₂S does not.

Assertion (A): Real gases deviate from ideal behavior at high pressure. Reason (R): At high pressure, the molecular volume becomes significant compared to container volume.