Pakistan MCQs

The system consumes some added reactant.
The shift reduces the imposed concentration change.

A Brønsted-Lowry base accepts H+.
It forms its conjugate acid.

The reaction produces more product to replace what was removed.
This is an application of Le Chatelier's principle.

Lewis theory focuses on electron-pair transfer.
Many metal ions and electron-deficient molecules act as Lewis acids.

Higher pressure favors the side occupying less gas volume.
That is usually the side with fewer gas moles.

Lewis bases donate a lone pair to form a coordinate bond.
Ammonia is a common example.

A catalyst lowers activation energies for both directions.
It speeds equilibration without changing the equilibrium position.

An acid forms its conjugate base after donating H+.
A base forms its conjugate acid after accepting H+.

Temperature alters the balance between forward and reverse energetics.
K is constant only at a specified temperature.

Strength refers to extent of ionization, not concentration.
Strong acids produce hydronium ions nearly completely.

Heat release gives a negative enthalpy sign.
-250 kJ divided by 2 mol equals -125 kJ/mol.

Weak-acid solutions contain both ionized and unionized forms.
They establish an equilibrium in water.