Chemical Kinetics And Nuclear Chemistry - Physical Chemistry - Chemistry Previous Year Questions

Fill in the blanks:

(A) \(_{92}^{235}\)U + \(_{0}^{1}\)n \(\to\) \(_{52}^{137}\)A + \(_{40}^{97}\)B + ____________.

(B) \(_{34}^{82}\)Se \(\to\) 2 \({}_{ - 1}{e^0}\) + __________.

For the following reaction

2X(g) \(\to\) 3Y(g) + 2Z(g)

assuming ideal gas conditions, the data for change of partial pressure with time is as follows:

$$\begin{array}{llll} \[\hline \text { Time (in min) } & 0 & 100 & 200 \\\] \[\hline \begin{array}{l}\] \[\text { Partial pressure of X } \\\] \[\text { (in mm of Hg) }\] \end{array} & 800 & 400 & 200 \end{array}$$

Calculate

(A) Order of reaction.

(B) Rate constant.

(C) Time taken for 75% completion of reaction.

(D) Total pressure of the reaction mixture when \(p_x=700\) mm.

$$\text { Match Column I with Column II : }$$

For a reversible reaction $R \rightleftharpoons P$, at constant temperature, both the forward and the backward reactions are first order elementary reactions with rate constants $k_{{f}}$ and $k_{{b}}$, respectively. At time zero, the concentration of $R$ is $[R]_0$ and the concentration of $P$ is zero. At any given time, $[R]$ and $[P]$ are the concentrations of $R$ and $P$, respectively. If $k_{{b}} = 4k_{{f}}$, the correct graphical representation of the reaction is