Respuesta :
Answer:
k₂ = 4.06 x 10⁻² s⁻¹.
Explanation:
- From Arrhenius law: K = Ae(-Ea/RT)
where, K is the rate constant of the reaction.
A is the Arrhenius factor.
Ea is the activation energy.
R is the general gas constant.
T is the temperature.
- At different temperatures:
ln(k₂/k₁) = Ea/R [(T₂-T₁)/(T₁T₂)]
k₁ = 5.8 × 10⁻³ s⁻¹, k₂ = ??? , Ea = 33600 J/mol, R = 8.314 J/mol.K, T₁ = 298.0 K, T₂ = 348.0 K.
- ln(k₂/5.8 × 10⁻³ s⁻¹) = (33600 J/mol / 8.314 J/mol.K) [(348.0 K - 298.0 K) / (298.0 K x 348.0 K)] = (4041.37) (4.82 x 10⁻⁴) = 1.9479.
- Taking exponential of both sides:
(k₂/5.8 × 10⁻³ s⁻¹) = 7.014.
∴ k₂ = 4.06 x 10⁻² s⁻¹.
The study of chemicals and bonds is called chemistry. There are different types of elements and are metals and nonmetals,
The correct answer to the question is k₂ = 4.06 x 10⁻² s⁻¹.
What is Arrhenius law?
- The Arrhenius equation is a formula for the temperature dependence of reaction rates
From Arrhenius law:
[tex]K = Ae(\frac{-Ea}{RT})[/tex] where,
- K is the rate constant of the reaction.
- A is the Arrhenius factor.
- Ea is the activation energy.
- R is the general gas constant.
- T is the temperature.
At different temperatures:
[tex]ln\frac{k_2}{k_1} = \frac{Ea}{R}\frac[{(T_2-T_1)}{(T_1T_)}[/tex]
All the data is given as follows:-
- k₁ = 5.8 × 10⁻³ s⁻¹,
- Ea = 33600 J/mol,
- R = 8.314 J/mol.K,
- T₁ = 298.0 K
- T₂ = 348.0 K.
[tex]ln(\frac{k_2}{5.8 * 10^{-3}}) = \frac{33600}{8.314} *\frac{(348.0 K - 298.0 K)}{(298.0 K* 348.0 K)} \\\\= (4041.37) (4.82 x 10^{-4}) = 1.9479.[/tex]
Taking exponential of both sides:
[tex]\frac{k_2}{5.8* 10^{-3}}\\ \\= 7.014.[/tex]
Hence, the correct answer is k₂ = 4.06 x 10⁻² s⁻¹.
For more information about the rate constant, refer to the link:-
https://brainly.in/question/9531558
