The rate constant for a certain reaction is measured at two different temperatures:
1 answer:
Answer: The activation energy Ea for this reaction is 22689.8 J/mol
Explanation:
According to Arrhenius equation with change in temperature, the formula is as follows.
= rate constant at temperature
=
= rate constant at temperature
=
= activation energy = ?
R= gas constant = 8.314 J/kmol
= temperature =
= temperature =
Putting in the values ::
The activation energy Ea for this reaction is 22689.8 J/mol
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Answer:
ν = 5,765x10¹⁴ Hz
λ = 520 nm
230,0 kJ/mole
Explanation:
To convert energy yo frequency you need to use:
E = hν
Where E is energy (3,820x10⁻¹⁹ J)
h is Planck's constant (6,626x10⁻³⁴ Js)
And ν is frequency, replacing ν = 5,765x10¹⁴ s⁻¹ ≡ 5,765x10¹⁴ Hz
To convert frequency to wavelength:
c = λν
Where s is speed of light (2,998x10⁸ ms⁻¹)
ν is frequency (5,765x10¹⁴ s⁻¹)
And λ is wavelength, replacing: λ = 5,200x10⁻⁷ ≡ 520 nm
If 1 photon produce 3,820x10⁻¹⁹ J, in mole of photons produce:
3,820x10⁻¹⁹ J × = 230040 J/mole ≡ 230,0 kJ/mole
I hope it helps!