Q. No.In the presence of a catalyst, the heat evolved or absorbed during the reaction:
1.
Increases.
2.
Decreases.
3.
Remains unchanged.
4.
May increase or decrease.
| 1. | Determining the rate constant at standard temperature. |
| 2. | Determining the rate constant at two temperatures. |
| 3. | Determining probability of collision. |
| 4. | Using the catalyst. |
The correct statement based on the graph below is:
| 1. | The activation energy of the forward reaction is E1 + E2 and the product is less stable than reactant. |
| 2. | The activation energy of the forward reaction is E1 + E2 and the product is more stable than the reactant. |
| 3. | The activation energy of both forward and backward reaction is E1 + E2 and reactant is more stable than the product. |
| 4. | The activation energy of the backward reaction is E1 and the product is more stable than reactant. |
Consider the first-order gas-phase decomposition reaction given below.
A(g) → B(g) + C(g)
The initial pressure of the system before the decomposition of A was . After the lapse of time t, the total pressure of the system increased by X units and became . The rate constant k for the reaction is:
| 1. | 2. | ||
| 3. | 4. |
Consider the Arrhenius equation given below and choose the correct option:
| 1. | Rate constant increases exponentially with increasing activation energy and decreasing temperature. |
| 2. | Rate constant decreases exponentially with increasing activation energy and increasing temperature. |
| 3. | Rate constant increases exponentially with decreasing activation energy and decreasing temperature. |
| 4. | Rate constant increases exponentially with decreasing activation energy and increasing temperature. |
True statement among the following is:
| 1. | The rate of a reaction decreases with the passage of time as the concentration of reactants decreases. |
| 2. | The rate of a reaction is the same at any time during the reaction. |
| 3. | The rate of a reaction is independent of temperature change. |
| 4. | The rate of a reaction decreases with an increase in the concentration of the reactants. |
The correct expression for the rate of reaction given below is:
\(5 \mathrm{Br}^{-}(\mathrm{aq})+\mathrm{BrO}_3^{-}(\mathrm{aq})+6 \mathrm{H}^{+}(\mathrm{aq}) \rightarrow 3 \mathrm{Br}_2(\mathrm{aq})+3 \mathrm{H}_2 \mathrm{O}(\mathrm{l})\)
| 1. | \(\frac{\Delta\left[B r^{-}\right]}{\Delta t}=5 \frac{\Delta\left[H^{+}\right]}{\Delta t} \) | 2. | \(\frac{\Delta\left[\mathrm{Br}^{-}\right]}{\Delta t}=\frac{6}{5} \frac{\Delta\left[\mathrm{H}^{+}\right]}{\Delta t} \) |
| 3. | \(\frac{\Delta[\mathrm{Br^-}]}{\Delta t}=\frac{5}{6} \frac{\Delta\left[\mathrm{H}^{+}\right]}{\Delta t} \) | 4. | \(\frac{\Delta\left[\mathrm{Br}^{-}\right]}{\Delta t}=6 \frac{\Delta\left[\mathrm{H}^{+}\right]}{\Delta t}\) |
Rate law for the reaction \(A+2 B \rightarrow C\) is found to be
Rate = k[A][B]
If the concentration of reactant 'B' is doubled, keeping the concentration of A constant, then the value of the rate of the reaction will be:
| 1. | The same. | 2. | Doubled. |
| 3. | Quadrupled. | 4. | Halved. |
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