At constant temperature and volume, X decomposes as 2X(g) $$\to$$ 3Y(g) + 2Z(g); P_x is the partial pressure of X.
(i) What is the order of the reaction to X?
(ii) Find the rate constant
(iii) Find the time for 75% completion of the reaction.
(iv) Find the total pressure when pressure of X is 700 mm of Hg

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.

For the given reactions, A + B $$\to$$ Products, following data were obtained
(a) Write the rate law expression
(b) Find the rate constant