The rate constants of reaction at 500 K and 700 K are 0.02 s-1 and 0.07 s-1 respectively. The value of A is

Question

The rate constants of reaction at 500 K and 700 K are 0.02 s-1 and 0.07 s-1 respectively. The value of A is (A) 2  (B)  4 (C)  1.61  (D) 3.5

Tardigrade Admin · Accepted Answer

log (k2/k1 )= (Ea/2.303 R) [(T2-T1/T1T2)] log (0.07/0,02)=[(Ea/2.303×8.314 Jk-1mol -1)][(700-500/700×500)] 0.544 =Ea×5.714×10-4 /19.15 Ea=0.544×19.15 5.714×10-4 = 18231.7J Since k=A e-Ed / R T 0.02=A e-18231.7 / 8.314 × 500 A=0.02 / 0.012=1.61

Q. The rate constants of reaction at $500 K$ and $700 K$ are $0.02 s^{- 1}$ and $0.07 s^{- 1}$ respectively. The value of $A$ is

$2$

$4$

$1.61$

$3.5$

Q. The rate constants of reaction at 500K and 700K are 0.02s−1 and 0.07s−1 respectively. The value of A is

2

4

1.61

3.5

logk1​k2​​=2.303REa​​[T1​T2​T2​−T1​​] log0,020.07​=[2.303×8.314Jk−1mol−1Ea​​][700×500700−500​] 0.544=Ea​×5.714×10−4/19.15 Ea​=0.544×19.155.714×10−4=18231.7J Since k=Ae−Ed​/RT 0.02=Ae−18231.7/8.314×500 A=0.02/0.012=1.61

Q. The rate constants of reaction at $500 K$ and $700 K$ are $0.02 s^{- 1}$ and $0.07 s^{- 1}$ respectively. The value of $A$ is

$2$

$4$

$1.61$

$3.5$