The decomposition of NH3 on a platinum surface is a zero-order reaction. The rates of production of N2 and H2
will be respectively:
(given ; k = 2.5 × 10–4 mol–1 L s–1 )
1. 2.5 x 10-4 mol L-1 s-1 and 5.5 x 10-4 mol L-1 s-1
2. 2.5 x 10-4 mol L-1 s-1 and 7.5 x 10-4 mol L-1 s-1
3. 1.5 x 10-4 mol L-1 s-1 and 4.5 x 10-4 mol L-1 s-1
4. 0.5 x 10-4 mol L-1 s-1 and 3.5 x 10-4 mol L-1 s-1
The rate equation of a reaction is expressed as, Rate = \(k(P_{CH_{3}OCH_{3}})^{\frac{3}{2}}\)
(Unit of rate = bar min-1)
The units of the rate constant will be:
1. bar1/2 min
2. bar2 min-1
3. bar-1min-2
4. bar-1/2min-1
The factor(s) that affect the rate of a chemical reaction is/are:
1. Concentration/Pressure of reactants.
2. Temperature.
3. Presence of a catalyst.
4. All of the above.
t/s | 0 | 30 | 60 | 90 |
[Ester]/mol L-1 | 0.55 | 0.31 | 0.17 | 0.085 |
A reaction is first-order with respect to A and second-order with respect to B. The concentration of B is increased three times. The new rate of the reaction would:
1. | Decrease 9 times | 2. | Increase 9 times |
3. | Increase 6 times | 4. | Decrease 6 times |
In a reaction between A and B, the initial rate of reaction (r0) was measured for different initial concentrations of A and B as given below:
A / mol L-1 | 0.20 | 0.20 | 0.40 |
B / mol L-1 | 0.30 | 0.10 | 0.05 |
ro / mol L-1 s-1 | 5.07 x 10-5 | 5.07 x 10-5 | 1.43 x 10-4 |
The order of the reaction with respect to A and B would be:
1. | The order with respect to A is 0.5 and with respect to B is zero. |
2. | The order with respect to A is 1 and with respect to B is 0.5 |
3. | The order with respect to A is 2 and with respect to B is 1 |
4. | The order with respect to A is 1.5 and with respect to B is zero |
For a reaction, 2A + B → C + D, the following observations were recorded:
Experiment | [A]/mol L-1 | [B]/mol L-1 | Initial rate of formation of D/mol L-1 min-1 |
I | 0.1 | 0.1 | 6.0 x 10-3 |
II | 0.3 | 0.2 | 7.2 x 10-2 |
III | 0.3 | 0.4 | 2.88 x 10-1 |
IV | 0.4 | 0.1 | 2.40 x 10-2 |
The rate law applicable to the above mentioned reaction would be:
1. Rate = k[A]2[B]3
2. Rate = k[A][B]2
3. Rate = k[A]2[B]
4. Rate = k[A][B]
For the reaction , rate = with k = and . The initial rate of the reaction will be :
1. 0.04 mol
2. 8
3. 8
4. 8 mol
Given that . The dimension of the rate constant in the given rate law is -
1.
2.
3.
4.
Consider the following rate expression.
The order of reaction and dimension of the rate constant are, respectively-
1. ; k =
2. 3; k =
3. ; k =
4. ; k =