1. | \(\dfrac{-\Delta[\mathrm{H}I]}{\Delta t}=\dfrac{2 \Delta\left[\mathrm{H}_2\right]}{\Delta t}\) | 2. | \(\dfrac{-\Delta[\mathrm{HI}]}{\Delta t}=\dfrac{4\Delta\left[\mathrm{I}_2\right]}{\Delta t}\) |
3. | \(\dfrac{-\Delta[\mathrm{HI}]}{\Delta t}=\dfrac{4 \Delta\left[\mathrm{H}_2\right]}{\Delta t}\) | 4. | \( \dfrac{-\Delta[\mathrm{H}]}{\Delta t}=\dfrac{\Delta\left[\mathrm{H}_2\right]}{\Delta t}\) |
1. | \(-\Delta [A] \over \Delta t\) | 2. | \(-3\Delta [A] \over 2\Delta t\) |
3. | \(-2\Delta [A] \over 3\Delta t\) | 4. | \(\Delta [A] \over \Delta t\) |
For the reaction, 2A → B, rates= k[A]2. If the concentration of reactant is doubled, then the:
(a) | rate of reaction will be doubled. |
(b) | rate constant will remain unchanged, however rate of reaction is directly proportional to the rate constant. |
(c) | rate constant will change since the rate of reaction and rate constant are directly proportional to each other. |
(d) | rate of reaction will increase by four times. |
Identify the set of correct statements & choose the correct answer from the options given below:
1. | (a) and (c) only | 2. | (a) and (b) only |
3. | (b) and (d) only | 4. | (c) and (d) only |
1. | 1 × 10–2 mol L–1 s–1 and 30 × 10–2 mol L–1 |
2. | 10 × 10–2 mol L–1 s–1 and 10 × 10–2 mol L–1 |
3. | 1 × 10–2 mol L–1 s–1 and 10 × 10–2 mol L–1 |
4. | 10 × 10–2 mol L–1 s–1 and 30 × 10–2 mol L–1 |
For the chemical reaction the correct option is:
1.
2.
3.
4.