At 345 K, the half life for the decomposition of a sample of a gaseous compound initially at 55.5 kPa was 340 s. When the pressure was 27.8 kPa, the half life was found to be 170 s. The order of the reaction is ____________. [integer answer]

For a reaction taking place in three steps at same temperature, overall rate constant $\mathrm{K}=\frac{\mathrm{K}_1 \mathrm{~K}_2}{\mathrm{~K}_3}$. If and are 40, 50 and respectively, the overall is ________ .

The number of given statement/s which is/are correct is __________.

(A) The stronger the temperature dependence of the rate constant, the higher is the activation energy.

(B) If a reaction has zero activation energy, its rate is independent of temperature.

(C) The stronger the temperature dependence of the rate constant, the smaller is the activation energy.

(D) If there is no correlation between the temperature and the rate constant then it means that the reaction has negative activation energy.

During Kinetic study of reaction $\mathrm{2 A+B \rightarrow C+D}$, the following results were obtained :

Catalyst A reduces the activation energy for a reaction by 10 kJ mol^$-$1 at 300 K. The ratio of rate constants, ${{{}^kT,\,Catalysed} \over {{}^kT,\,Uncatalysed}}$ is e. The value of x is ___________. [nearest integer]

A flask is filled with equal moles of A and B. The half lives of A and B are 100 s and 50 s respectively and are independent of the initial concentration. The time required for the concentration of A to be four times that of B is ___________ s.

(Given : ln 2 = 0.693)

The rate constant for a first order reaction is given by the following equation:

$\ln k = 33.24 - {{2.0 \times {{10}^4}\,K} \over T}$

It has been found that for a chemical reaction with rise in temperature by 9 K the rate constant gets doubled. Assuming a reaction to be occurring at 300 K, the value of activation energy is found to be ____________ kJ mol^$-$1. [nearest integer]

(Given ln10 = 2.3, R = 8.3 J K^$-$1 mol^$-$1, log 2 = 0.30)

The activation energy of one of the reactions in a biochemical process is 532611 J mol^$-$1. When the temperature falls from 310 K to 300 K, the change in rate constant observed is k₃₀₀ = x $\times$ 10^$-$3 k. The value of x is ____________.

The number of correct statement/s involving equilibria in physical processes from the following is ________

(A) Equilibrium is possible only in a closed system at a given temperature.

(B) Both the opposing processes occur at the same rate.

(C) When equilibrium is attained at a given temperature, the value of all its parameters became equal.

(D) For dissolution of solids in liquids, the solubility is constant at a given temperature.

The following concentrations were observed at $500 \mathrm{~K}$ for the formation of $\mathrm{NH}_3$ from and . At equilibrium ; and . Equilibrium constant for the reaction is ________.

For the reaction $\mathrm{N}_2 \mathrm{O}_{4(\mathrm{~g})} \rightleftarrows 2 \mathrm{NO}_{2(\mathrm{~g})}, \mathrm{K}_{\mathrm{p}}=0.492 \mathrm{~atm}$ at for the reaction at same temperature is _________ .

An acidified manganate solution undergoes disproportionation reaction. The spin-only magnetic moment value of the product having manganese in higher oxidation state is _____________ B.M. (Nearest integer)

The equilibrium composition for the reaction $\mathrm{PCl}_{3}+\mathrm{Cl}_{2} \rightleftharpoons \mathrm{PCl}_{5}$ at is given below: