Question

Statement-1: The value of van der Waal's constant $\left(a\right)$ is larger for ammonia than for nitrogen.
Statement-2: Hydrogen bonding is present in ammonia.

• A. Statement-1 is True, Statement-2 is True; Statement-2 is a correct expalnation for Statment-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. Statement-1 is False, Statement-2 is True

Answer 1

The correct option is A Statement-1 is True, Statement-2 is True; Statement-2 is a correct expalnation for Statment-1.

The value of van der Waal's constant $\left(a\right)$ is directly proportional to the force of attraction between the molecules. $N{H}_3$ has hydrogen bonding whereas nitrogen has London dispersion force. As hydrogen bonding is stronger than London dispersion forces, ammonia has a larger force of attraction than nitrogen.
Thus, Statement-1 is True, Statement-2 is True; Statement-2 is a correct explanation for Statement-1.