A light photon with a frequency of at least 0.0373 × 1016 Hz is required to split apart diiodine according to the equation:
I2(g) → 2I(g)
Calculate the energy (kJ) required to break apart a mole of diiodine. Express answer in scientific notation.
I got 2.47 * 10^-22 but it's incorrect.
I used the equation: E = (h)(v)
h = 6.624*10^-34 J*s
f = 3.73*10^14 s^-1
h*f = 2.47*10^-19 joule
= 2.47*10^-22 kJ
That is the energy need to break apart a molecule, NOT a mole. You must multiply that number by Avogadro's number. You should get about 149 kJ/mole
To calculate the energy required to break apart a mole of diiodine (I2), you are correct in using the equation E = hv, where E represents the energy, h is the Planck's constant, and v is the frequency of the light photon.
The energy required to break apart a mole of diiodine can be calculated by multiplying the Avogadro's number (6.022 × 10^23) with the energy required to break apart a single diiodine molecule. This can be determined by multiplying the frequency of the light photon (v) with the Planck's constant (h).
Given the frequency of the light photon as 0.0373 × 10^16 Hz, and the Planck's constant (h) as 6.626 × 10^-34 J·s, we can calculate the energy required for a single diiodine molecule:
E = hv = (6.626 × 10^-34 J·s)(0.0373 × 10^16 Hz)
= 2.4698 × 10^-17 J
Now, to calculate the energy required to break apart a mole (6.022 × 10^23) of diiodine molecules, we multiply the energy calculated above by Avogadro's number:
Energy required = (6.022 × 10^23)(2.4698 × 10^-17 J)
= 1.4863 × 10^7 J
To express this answer in scientific notation, we can convert the answer from joules (J) to kilojoules (kJ):
1 J = 0.001 kJ
Therefore, the energy required to break apart a mole of diiodine is:
1.4863 × 10^7 J = 1.4863 × 10^4 kJ
Hence, the correct answer is 1.4863 × 10^4 kJ, not 2.47 × 10^-22 as you obtained earlier.