Consider two reactions having same Arrhenius factor A, but different energy of activation. (i) A arrow B; Ea1=20 kJ (ii) C arrow D; Ea2=30 kJ Both are at temperature 25° C If temperature in both reaction is increased slightly in such a way that change in temperature in both case is same than choose the correct options.

Question

Consider two reactions having same Arrhenius factor A, but different energy of activation. (i) A arrow B; Ea1=20 kJ (ii) C arrow D; Ea2=30 kJ Both are at temperature 25° C If temperature in both reaction is increased slightly in such a way that change in temperature in both case is same than choose the correct options. (A) The second reaction is faster (B) The second reaction is more sensitive towards temperature variation (C) If temperature increases, rate of first reaction increase more sharply (D) All the above are correct

Tardigrade Admin · Accepted Answer

Arrhenius equation; d(l n k)=(Ea/R T2)dT Here, T and dT same and positive d(l n k)α Ea lnk2-lnk1α Ea ln(K2/K1)α Ea So, if temperature increases, then rate of reaction having more Ea increases more sharply.

The second reaction is faster

The second reaction is more sensitive towards temperature variation

If temperature increases, rate of first reaction increase more sharply

All the above are correct

Arrhenius equation; d(lnk)=RT2Ea​​dT Here, T and dT same and positive d(lnk)αEa​ lnk2​−lnk1​αEa​ lnK1​K2​​αEa​ So, if temperature increases, then rate of reaction having more Ea​ increases more sharply.

Arrhenius equation;

$d (l nk) = \frac{E _{a}}{R T ^{2}} d T$

Here, T and dT same and positive

$d (l nk) α E_{a}$

$l n k_{2} - l n k_{1} α E_{a}$

$l n \frac{K _{2}}{K _{1}} α E_{a}$

So, if temperature increases, then rate of reaction having more $E_{a}$ increases more sharply.