Explanation

Reaction: CaCO3 + 2HCl -> CaCl2 + CO2 + H2O

Given:

CaCO3 = 50g

Actual CO2 = 14.52g

Step 1: Molar mass of CaCO3 = 100 g/mol

Moles of CaCO3 = 50 / 100 = 0.5 mole

Step 2: 1 mole CaCO3 gives 1 mole CO2

So 0.5 mole CaCO3 gives 0.5 mole CO2

Step 3: Molar mass of CO2 = 44 g/mol

Theoretical yield of CO2 = 0.5 x 44 = 22g

Step 4: Percentage yield = (Actual / Theoretical) x 100

= (14.52 / 22) x 100

= 66%

Theoretical yield = 22g

Percentage yield = 66%

Last verified on 25-10-2026

Explanation

• According to Le Chatelier’s principle, adding nitrogen increases the concentration of a reactant, causing the equilibrium to shift to the right.
• The forward reaction consumes nitrogen and hydrogen to produce ammonia (NH₃).
• Therefore, adding more nitrogen increases the amount of ammonia produced as the system reaches a new equilibrium.

Last verified on 25-10-2026

Explanation

• A basic buffer solution consists of a weak base and its conjugate acid.
• It resists changes in pH when small amounts of acid or base are added.
• Ammonia (NH₃) is a weak base.
• When hydrochloric acid (HCl) reacts with excess ammonia, it forms ammonium chloride (NH₄Cl), leaving some unreacted NH₃.
• The mixture contains a weak base (NH₃) and its conjugate acid (NH₄⁺), making it a basic buffer solution.

Last verified on 25-10-2026

Explanation

• A catalyst increases the rate of a chemical reaction by providing an alternative reaction pathway with lower activation energy.
• Activation energy is the minimum energy required for reactants to start a chemical reaction.
• Lower activation energy allows more particles to react successfully in a given time.

Last verified on 25-10-2026

Explanation

• The compound CH₃CH=CH–C≡CH contains five carbon atoms, so the parent name is “penta.”
• Numbering starts from the end nearest the triple bond, giving the triple bond position 1 and the double bond position 3.
• The correct IUPAC name is pent-3-en-1-yne.

Last verified on 25-10-2026