The equation `K= (6.5 xx 10^(12) s^(-1)) e^(-26000K//T)` is followed for the decomposition of compound A. The activation energy for the reaction is ___ kJ `mol^(-1)` . [nearest integer] (Given R= 8.314 J `K^(-1) mol^(-1)`)

The equilibrium constant for a reaction is 10 . What will be the value of DeltaG^(Θ) ? R=8.314 J K^(-1) mol^(-1), T=300 K .

For a reaction, the activation energy is zero. What is the value of rate constant at 300 K if k=1.6 xx 10^(6)s^(-1) at 280 K (R= 8.31 JK^(-1)mol^(-1)) ?

For the reaction A rarr B , the rate constant k (in s^(-1) ) is given by log_(10) k = 20.35 - ((2.47 xx 10^(3)))/(T) The energy of activation in kJ mol^(-1) is ________ . (Nearest integer) [Given : R = 8.314 J K^(-1) mol^(-1) ]

The kinetic energy of two moles of N_(2) at 27^(@) C is (R = 8.314 J K^(-1) mol^(-1))

The rate of a reaction doubles when the tempeature changes from 300 K to 310 K. Activation energy for the reaction is: (R = 8.314 JK^(-1) mol^(-1), log2 = 0.3010)

The decomposition of formic acid on gold surface follows first order kinetics. If the rate constant at 300 K is 1.0 xx 10 ^(-3) s ^(-1) and and the activation energy E _(a) =11,488 Kj mol ^(-1). the rate constant at 200 K is "________"xx 10 ^(-5) s ^(-1). (Round off to the Nearest Integer). (Given : R= 8.314 J mol ^(-1) K ^(-1))