For a reaction, activation energy Ea=0 and the rate constant at 200K is 1.6×106s-1. The rate constant at 400K will be- [Given that gas constant] R= 8.314 J K-1 mol-1

Question

For a reaction, activation energy Ea=0 and the rate constant at 200K is 1.6×106s-1. The rate constant at 400K will be- [Given that gas constant] R= 8.314 J K-1 mol-1 (A) 3.2 ×104 s-1 (B) 1.6 × 106 s-1 (C) 1.6 × 103 s-1 (D) 3.2 × 106 s-1

Tardigrade Admin · Accepted Answer

log((K2/K1)) = (E/2.303 R)((1/T1) - (1/T2)) Ea = 0 log((K2/K1)) = 0 (K2/K1) = 10° = 1 ⇒ K2 = K1 K2 = 1.6 × 106 s-1 at 400K

Q. For a reaction, activation energy E $_{a}$ =0 and the rate constant at 200K is 1.6×10 $^{6}$ s $^{- 1}$ . The rate constant at 400K will be-
[Given that gas constant]
R= 8.314 J K $^{- 1}$ mol $^{- 1}$

3.2 ×10 $^{4}$ s $^{- 1}$

1.6 × 10 $^{6}$ s $^{- 1}$

1.6 × 10 $^{3}$ s $^{- 1}$

3.2 × 10 $^{6}$ s $^{- 1}$

$l o g (\frac{K _{2}}{K _{1}}) = \frac{E}{2.303 R} (\frac{1}{T _{1}} - \frac{1}{T _{2}})$
$E_{a} = 0$
$l o g (\frac{K _{2}}{K _{1}}) = 0$
$\frac{K _{2}}{K _{1}} = 1 0^{\circ} = 1$
$\Rightarrow K_{2} = K_{1}$
$K_{2} = 1.6 \times 1 0^{6} s^{- 1}$ at $400 K$

Q. For a reaction, activation energy Ea​=0 and the rate constant at 200K is 1.6×106s−1. The rate constant at 400K will be- [Given that gas constant] R= 8.314 J K−1 mol−1

3.2 ×104 s−1

1.6 × 106 s−1

1.6 × 103 s−1

3.2 × 106 s−1