1. | –1.5 | 2. | 1.5 |
3. | 0.5 | 4. | 2.5 |
Experiment | [A] | [B] | Rate (mole litre-1 min-1) |
1. | 0.01 | 0.01 | 2 × 10-4 |
2. | 0.02 | 0.01 | 4 × 10-4 |
3. | 0.01 | 0.02 | 8 × 10-4 |
1. | Rate = K [A]2 [B] and litre2 mole-2 min-1 |
2. | Rate = K [A]3 and litre2 mole-2 min-1 |
3. | Rate = K [A] [B]2 and litre mole-1 min-1 |
4. | Rate = K [A] [B]2 and litre2 mole-2 min-1 |
1. | \(\small{CH_3COOC_2H_5 + NaOH \rightarrow CH_3COONa + C_2H_5OH}\) |
2. | \(\small{CH_3COOC_2H_5 + H_2O \xrightarrow{H^+} CH_3COOH + C_2H_5OH}\) |
3. | \(C_{12}H_{22}O_{11}+ H_2O \xrightarrow{H^+} C_6H_{12}O_6+ C_6H_{12}O_6\\ (cane~ sugar)~~~~~~~~~~~~~~~~(glucose)~~~~~(Fructose)\) |
4. | Both 2 and 3 |
The elementary step of the reaction, \(2 \mathrm{Na}+\mathrm{Cl}_2\rightarrow2 \mathrm{NaCl}\) is found to follow 3rd order kinetics. Its molecularity is:
1. One
2. Two
3. Three
4. Four
H2 gas is absorbed on the metal surface like gold, tungsten, etc. This follows ________ order reaction:
1. | Third | 2. | Second |
3. | Zero | 4. | First |
Half-life of substance A following first order kinetics is 5 days. Starting with 100g of A, the amount left after 15 days will be:
1. 25 g
2. 50 g
3. 12.5 g
4. 6.25 g
1. | large value of k indicates fast reactions. |
2. | The value of k is independent of the concentration of reactants |
3. | The value of k is independent of the concentration of products |
4. | The value of the rate constant, k, as the name suggests is always constant for a particular reaction at all temperatures. |