The slope of Arrhenius Plot ( ln k v / s (1/ T )) of first order reaction is -5 × 103 K. The value of E a of the reaction is. Choose the correct option for your answer. [. Given .R =8.314 JK -1 mol -1]

Question

The slope of Arrhenius Plot ( ln k v / s (1/ T )) of first order reaction is -5 × 103 K. The value of E a of the reaction is. Choose the correct option for your answer. [. Given .R =8.314 JK -1 mol -1] (A) 41.5 kJ mol -1 (B) 83.0 kJ mol -1 (C) 166 kJ mol -1 (D) -83 kJ mol -1

Tardigrade Admin · Accepted Answer

K = Ae -(Ea/R T) undersety ln K = undersetC ln A - undersetm( E a / R ) ⋅ undersetx(1/ T ) Slope =-( E a / R ) -( E a / R )=-5 × 103 K E a =5 × 8.314 J K -1 mole -1 × 103 K

Q. The slope of Arrhenius Plot $(ln k v / s \frac{1}{T})$ of first order reaction is $- 5 \times 1 0^{3} K$ . The value of $E_{a}$ of the reaction is. Choose the correct option for your answer. $[$ Given $R = 8.314 J K^{- 1} m o l^{- 1}]$

$41.5 k J m o l^{- 1}$

$83.0 k J m o l^{- 1}$

$166 k J m o l^{- 1}$

$- 83 k J m o l^{- 1}$

$K = A e^{- \frac{E _{a}}{RT}}$
$y ln K = C ln A - m \frac{E _{a}}{R} \cdot x \frac{1}{T}$
Slope $= - \frac{E _{a}}{R}$
$- \frac{E _{a}}{R} = - 5 \times 1 0^{3} K$
$E_{a} = 5 \times 8.314 J K^{- 1} m o l e^{- 1} \times 1 0^{3} K$

Q. The slope of Arrhenius Plot (lnkv/sT1​) of first order reaction is −5×103K. The value of Ea​ of the reaction is. Choose the correct option for your answer. [ Given R=8.314JK−1mol−1]

41.5kJmol−1

83.0kJmol−1

166kJmol−1

−83kJmol−1