NEET Chemistry - MCQ Practice Questions

A first-order reaction has a rate constant k = 0.693 s⁻¹. Calculate the half-life of this reaction.

Which of the following is true for an endothermic reaction?

For the equilibrium PCl₅(g) ⇌ PCl₃(g) + Cl₂(g), Kc = 1.8 at 298 K. If initial concentration of PCl₅ is 1 M, find [PCl₃] at equilibrium when dissociation is 30%.

The hydration enthalpy of an ion depends on which of the following factors?

In electrochemistry, what does the cell potential (E°cell) indicate?

A solution has pH = 4. What is the concentration of H⁺ ions?

For a reversible adiabatic process of an ideal gas, which statement is correct?

The standard cell potential for a cell is E° = 1.10 V. Calculate ΔG° (F = 96500 C/mol, n = 2):

For the reaction: A → B, if the order is 2 and rate constant k = 0.5 L·mol⁻¹·s⁻¹, find the half-life when initial concentration is 2 M.

The relationship between Kp and Kc for the reaction N₂O₄(g) ⇌ 2NO₂(g) is:

What is the entropy change when 18 g of ice at 273 K is converted to water at 273 K? (ΔfusH = 6 kJ/mol)

A buffer solution contains 0.1 M acetic acid and 0.1 M sodium acetate. If Ka = 1.8 × 10⁻⁵, calculate the pH:

In electrolysis, if 2 moles of electrons are transferred, how many moles of Cu will be deposited from CuSO₄ solution? (Atomic mass of Cu = 64)

For the reaction 2NO(g) + O₂(g) → 2NO₂(g), if the reaction rate increases by a factor of 8 when [NO] is doubled and [O₂] is kept constant, what is the order of reaction with respect to NO?

At 298 K, the vapor pressure of water is 23.8 mmHg. What is the mole fraction of water vapor in saturated air at this temperature?

For the reaction: N₂O₄(g) ⇌ 2NO₂(g), ΔH = 58 kJ/mol. If pressure is increased at constant temperature, the equilibrium will:

Which electrochemical cell cannot be recharged?

At 273 K, 1 mole of an ideal gas occupies 22.4 L. What will be its volume at 546 K and same pressure?

The rate constant for a first-order reaction is 0.693 min⁻¹. What is its half-life?

When 50 mL of 0.1 M HCl is mixed with 50 mL of 0.1 M NaOH, the resulting solution will have: