Graph of logK and 1/T was given for which valuue of slope is -10000 K if T is 500K and rate constant is `10^(-5)` at which temperature value rate constant will be `10^-4`

For a reaction graph between logK vs 1/T is as with slope = -10,000. At temperature 500K rate constant k = 10^(-5) . Find the temperature in K at which rate constant = 10^(-4)

Which of the following graph is incorrect for variation of rate constant (K) with temperature for a reaction obeying Arrhenius equation ?

K is rate constant at temp T then value of underset(Ttooo)lim log K is equal to :-

The activation energy of a reaction is zero. Its rate constant at 280 K is 16 xx 10^(-6) s^(-1) the rate constant at 300k is

Which one of the following given graphs represents the variation of rate constant (k) with temperature (t) for an endothermic reaction ?

[A] = reactant concentration at time 't', k = rate constant

Which one of the following given graphs represents the variation of rate constant (k) with temperature (f) for an endothermic reaction ?