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Chapter 7: Chemical Kinetics & Enzyme Catalysis (Set-4)
Enzymes are generally A carbohydrates B proteins C lipids D salts Explanation Most enzymes are globular proteins (some RNA also acts as enzyme—ribozymes, but basic concept: proteins). The region where substrate binds to enzyme is called A coenzyme site B active site C allosteric site D prosthetic site only Explanation Active site has specific shape…
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Chapter 7: Chemical Kinetics & Enzyme Catalysis (Set-3)
Arrhenius equation is A k = [A]₀ − kt B k = Ae^(−Ea/RT) C 1/[A] = 1/[A]₀ + kt D log[A] = log[A]₀ − (k/2.303)t Explanation It relates rate constant to temperature and activation energy. In Arrhenius equation, A is called A activation energy B frequency (pre-exponential) factor C gas constant D rate of reaction…
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Chapter 7: Chemical Kinetics & Enzyme Catalysis (Set-2)
Integrated rate equation for zero-order reaction is A [A] = [A]₀e^(-kt) B [A] = [A]₀ − kt C 1/[A] = 1/[A]₀ + kt D log[A] = log[A]₀ − kt Explanation Zero order gives linear decrease of concentration with time. For a first-order reaction, t½ equals A 0.693k B 2.303/k C 0.693/k D 1/k² Explanation Half-life…
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Chapter 7: Chemical Kinetics & Enzyme Catalysis (Set-1)
The rate of a chemical reaction is defined as the change in A temperature per unit time B concentration per unit time C pressure per unit volume D energy per unit mass Explanation Rate measures how fast reactant concentration decreases or product concentration increases with time. The SI unit of rate of reaction is A…
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Chapter 6: Redox & Electrochemistry (Set-4)
Corrosion of iron is an example of A spontaneous redox reaction B non-spontaneous reaction C electrolytic reaction only D neutralization reaction Explanation Corrosion occurs naturally without external energy. Oxidation number of sulfur in Na₂S₂O₃ is A +2 B +4 C +6 D average +2 Explanation In thiosulfate, the two sulfur atoms are not equivalent (one…
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Chapter 6: Redox & Electrochemistry (Set-3)
Oxidation number of chromium in K₂Cr₂O₇ is A +3 B +4 C +6 D +7 Explanation Let oxidation number of Cr = x 2(+1) + 2x + 7(−2) = 0 2 + 2x − 14 = 0 → 2x = 12 → x = +6 Oxidation number of nitrogen in NH₄⁺ ion is A −1…
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Chapter 6: Redox & Electrochemistry (Set-2)
When balancing redox reactions by the ion–electron method, the key idea is to split the overall reaction into oxidation and reduction half-reactions so that electron transfer can be balanced explicitly. A Split into half-reactions B Add catalyst first C Remove spectators first D Balance oxygen last Explanation The ion–electron method becomes systematic by separating oxidation…
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Chapter 6: Redox & Electrochemistry (Set-1)
A redox reaction is one in which A only oxidation occurs B only reduction occurs C oxidation and reduction occur simultaneously D atoms are neither oxidized nor reduced Explanation Oxidation and reduction are complementary; one cannot occur without the other. Oxidation is defined as A gain of electrons B loss of electrons C gain of…
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Chapter 5: Solutions, Colligative Properties, Surface Chemistry & Colloids (Set-4)
Henry’s law relates solubility of a gas in a liquid to A temperature only B pressure of the gas C volume of the liquid D density of the gas Explanation Henry’s law: solubility of gas ∝ partial pressure of the gas above the solution. Solubility of most gases in water decreases with A decrease in…
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Chapter 5: Solutions, Colligative Properties, Surface Chemistry & Colloids (Set-3)
A non-volatile solute is added to a solvent. The vapor pressure of the solution A increases B decreases C remains same D becomes zero Explanation Addition of non-volatile solute reduces mole fraction of solvent, lowering vapor pressure. Relative lowering of vapor pressure is independent of A mole fraction of solute B nature of solute C…
