For a reaction Ea = 0 and k - 3.2 × 104 s-1 at 300 K. The value of k at 310 K would be :

Question

For a reaction Ea = 0 and k - 3.2 × 104 s-1 at 300 K. The value of k at 310 K would be : (A) 6.4 × 104 s-1 (B) 3.2 × 104 s-1 (C) 3.2× 108s-1 (D) 3.2 × 105 s-1

Tardigrade Admin · Accepted Answer

k=Ae-Ea/RT When Ea=0, k=A= constant ∴ k310=k300=3.2×104s-1

Q. For a reaction $E_{a} = 0$ and $k - 3.2 \times 1 0^{4} s^{- 1}$ at $300 K .$ The value of $k$ at $310 K$ would be :

$6.4 \times 1 0^{4} s^{- 1}$

$3.2 \times 1 0^{4} s^{- 1}$

$3.2 \times 1 0^{8} s^{- 1}$

$3.2 \times 1 0^{5} s^{- 1}$

$k = A e^{- E_{a / RT}}$
When $E_{a} = 0, k = A =$ constant
$∴ k_{310} = k_{300} = 3.2 \times 1 0^{4} s^{- 1}$

Q. For a reaction Ea​=0 and k−3.2×104s−1 at 300K. The value of k at 310K would be :

6.4×104s−1

3.2×104s−1

3.2×108s−1

3.2×105s−1