For the reaction

2A + B → 3C + D

An incorrect expression for the rate of reaction is:

1.

2. $-\frac{d\left[B\right]}{dt}$

3.

4. $-\frac{d\left[A\right]}{2dt}$

Subtopic:  Definition, Rate Constant, Rate Law |
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The following reaction was carried out at 300 K.

$2S{O}_{2}\left(g\right)+{O}_{2}\left(g\right)\to 2S{O}_{3}\left(g\right)$

The rate of formation of $S{O}_{3}$ is related to the rate of disappearance of ${O}_{2}$  by the following expression:

1. $-\frac{∆\left[{O}_{2}\right]}{∆t}=+\frac{1}{2}\frac{∆\left[S{O}_{3}\right]}{∆t}$

2. $-\frac{∆\left[{O}_{2}\right]}{∆t}=\frac{∆\left[S{O}_{3}\right]}{∆t}$

3. $-\frac{∆\left[{O}_{2}\right]}{∆t}=-\frac{1}{2}\frac{∆\left[S{O}_{3}\right]}{∆t}$

4. None of the above.

Subtopic:  Definition, Rate Constant, Rate Law |
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The correct expression for the rate of reaction given below is:

1.

2.

3.

4.

Subtopic:  Definition, Rate Constant, Rate Law |
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For a general reaction A $\to$ B, the plot of the concentration of A vs. time is given in the figure. The slope of the curve will be:

1. -k

2. -k/2

3. -k2

4. -k/3

Subtopic:  Definition, Rate Constant, Rate Law |
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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.

Subtopic:  Definition, Rate Constant, Rate Law |
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For the reaction,

${N}_{2}{O}_{5}\left(g\right)\to 2N{O}_{2}\left(g\right)+\frac{1}{2}{O}_{2}\left(g\right)$

the value of the rate of disappearance of ${\mathrm{N}}_{2}{\mathrm{O}}_{5}$ is given as . The rate of formation of  is given respectively as:

1. 6.25 x 10-3 mol L-1s-1 and 6.25 x 10-3 mol L-1s-1

2. 1.25 x 10-2 mol L-1s-1 and 3.125 x 10-3 mol L-1s-1${}^{}$

3. 6.25 x 10-3 mol L-1s-1 and 3.125 x 10-3 mol L-1s-1

4. 1.25 x 10-2 mol L-1s-1 and 6.25 x 10-3 mol L-1s-1

Subtopic:  Definition, Rate Constant, Rate Law |
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During the formation of ammonia by Haber's process N2+3H2 → 2NH3, the rate of appearance of NH3 was measured as 2.5 x 10-4 mol L-1 s-1. The rate of disappearance of H2 will be:

1. 2.5 x 10-4 mol L-1 s-1

2. 1.25 x 10-4 mol L-1 s-1

3. 3.75 x 10-4 mol L-1 s-1

4. 15.00 x 10-4 mol L-1 s-1

Subtopic:  Definition, Rate Constant, Rate Law |
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For the reaction, N2 + 3H2 $\to$ 2NH3, if$\frac{d\left[N{H}_{3}\right]}{dt}$=2 x 10-4 mol L-1 s-1, the value of would be:

1.

2.

3.

4.

Subtopic:  Definition, Rate Constant, Rate Law |
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The rate constant of a particular reaction has the dimensions of a frequency. The order of the reaction is:

1. Zero

2. First

3. Second

4. Fractional

Subtopic:  Definition, Rate Constant, Rate Law |
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The incorrect statement regarding the order of reaction is:

1.  Order is not influenced by the stoichiometric coefficient of the reactants.

2.  Order of reaction is the sum of power to the concentration terms of reactants to express the rate of reaction.

3. The order of reaction is always a whole number.

4.  Order can be determined by experiments only.

Subtopic:  Definition, Rate Constant, Rate Law |
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