`C_(4)H_(8)to2C_(2)H_(4)`. The rate constant is `2.84xx10^(-4)s^(-1)`. Calculate the time required to attain a molar ratio of the mixture, ethylene to cyclobutane is equal to `1:100`.

The rate constant at 0^(@)C is 7.87 xx 10^(-7)s^(-1) for a reaction whose energy of activation is 103 kJmol^(-1) Calculate the rate constant at 20^(@)C

The first order rate constant for the decomposition of ethyl iodide by the reaction. C_(2)H_(2)I (g)to C_(2)H_(4) (g)+ HI (g)at 600K is 1.60 xx10^(-5)s^(-1). It is energy of activation is 209 kJ/mol. Calculate the rate constant of the reaction at 700 K.

Assume that heat capacity of H_(2) O to be 4.2 xx 10^(3) J kg ^ (-1) K^(-1) and the latent heat of vapourisation of H_(2) O to be 22.5 xx 10^(5) J kg^(-1) . The amount of heat in joule required to heat 1 kg of water from 50^(@)C to 100^(@)C and then to convert into steam at 100^(@)C is

A_((g))+1/2B_((g))to2C+1/2D_((g)) The rate of disappearance of B is x. What is the rate of appearance of C?

For the reaction 2N_(2)O_(5)to4NO_(2)+O_(2) , rate and rate constant are 1.02xx10^(-4)M"sec"^(-1) and 3.4xx10^(-5)"sec"^(-1) respectively then concentration of N_(2)O_(5) at that time will be (in moles /lit)

The solubility product constant of Ag_(2)CrO_(4) and AgBr are 1.1xx10^(-12) and 5.0xx10^(-13) respectively. Calculate the ratio of the molarities of their saturated solutions.

K_(C) "for " H_(2) + 1//2 O_(2) rArr H_(2) O at 500 K is 2.4 xx 10^(47) . Now backward reaction is fovoured by

K_(C) "for " H_(2) + 1//2 O_(2) rArr H_(2) O at 500 K is 2.4 xx 10^(47) . Now backward reaction is fovoured by