Test: Chemical Kinetics(10 Nov) - JEE MCQ

The correct answer is Option A.

E represents the energy of activation which implies it is the energy below which colliding molecules will not react Arrhenius equation gives the dependence of the rate constant k of a chemical reaction on the absolute temperature T (in Kelvin), where A is the pre-exponential factor (or simply the prefactor), Ea is the activation energy, and R is the Universal gas constant:
By Arrhenius equation, k=Ae^-Ea/RT

The correct answer is option c
NO_(g)+Br_2(g)     ⇌NOBr_2(g)
NOBr2_(g)+NO_(g) 2NOBr_(g)[rate determining step]
Rate of the reaction (r)= K[NOBr₂][NO]
Where [NOBR²]=Kc[NO][Br2]
r=K.K_c.[NO][Br²][NO]
r=K’[NO]²[Br₂].
The order of the reaction with respect to
NO(g)=2.
 

The correct answer is Option C

The correct answer is Option C.

Now 2.303log10 
2.303log102 = 
∴
=53598.6 J 
=53.6 kJmol⁻¹