Tag: chemical reactions and equations

Quizzes (9) Questions (4)

Questions Related to chemical reactions and equations

Multiple choice chemistry chemical reactions and equations introduction to chemical kinetics understanding chemical kinetics rate of chemical reaction

Which statements are correct in terms of chemical kinetic stuides?

  1. The quenching of a reaction can be made by cooling the reaction mixture.

  2. The quenching of a reaction can be made by diluting the reaction mixture.

  3. The reaction is supposed to be completed if it is kept for long time or strongly heated.

  4. None of the above
Reveal answer Fill a bubble to check yourself
A,B,C Correct answer
Explanation

The quenching of a reaction can be made by cooling as well as diluting the reaction mixture. The reaction is supposed to be completed if it is kept for a long time or strongly heated. Quenching a reaction is used to deactivate any unreacted reagents. It is also done by adding an antisolvent to induce precipitation, and collecting or removing the solids.

Multiple choice chemistry chemical reactions and equations kinetic study of some first order reactions rate of chemical reaction endothermic and exothermic reactions

The rate constant for the reaction $2{N} _{2}{O} _{5}\rightarrow 4{N}{O} _{2}+{O} _{2}$, is $3.0\times 10^{-5}\sec^{-1}$. lf the rate is $2.40\times 10^{-5}$ mol litre $sec^{-1}$ then, the concentration of ${N} _{2}{O} _{5} ($in mol $litre^{-1})$ is:

  1. 1.4

  2. 1.2

  3. 0.04

  4. 0.8
Reveal answer Fill a bubble to check yourself
D Correct answer
Explanation

Rate constant $= 3 \times 10^{-5} sec^{-1}$


So, from it's unit it is clear that, it is a first order reaction.


For first order reaction the expression will be:
Rate $= K [N _{2}O _{5}]$
$[N _{2}O _{5}] = \dfrac{2.40 \times 10^{-5}}{3 \times 10^{-5}}$$=\dfrac{2.40}{3} = 0.8$

Multiple choice chemistry chemical reactions and equations kinetic study of some first order reactions rate of chemical reaction endothermic and exothermic reactions

For the reaction $2N _2O _5\, \rightarrow\, 4NO _2\, +\, O _2$, if $\displaystyle -\, \frac{d[N _2O _5]}{dt}\, =\, k _1[N _2O _5]$, $\displaystyle \frac{d[NO _2]}{dt}\, =\, k _2[N _2O _5]$, $\displaystyle \frac{d[O _2]}{dt}\, =\, k _3[N _2O _5]$.
What is the relation between $k _1, k _2$ and $k _3$?

  1. $k _1\, =\, k _2\, =\, k _3$
  2. $2k _1\, =\, k _2\, =\, 4k _3$
  3. $2k _1\ =\, 4k _2\, =\, k _3$

  4. None of the above
Reveal answer Fill a bubble to check yourself
B Correct answer
Explanation

As we know, for a reaction: $2N _2O _5\, \rightarrow\, 4NO _2\, +\, O _2$

$\displaystyle -\, \frac{1}{2}\, \frac{d[N _2O _5]}{dt}\, =\, \frac{1}{4}\, \frac{d[NO _2]}{dt}\, =\, \frac{d[O _2]}{dt}$

So, $2k _1\, =\, k _2\, =\, 4k _3.$