Nitrogen dioxide is one of the components of photochemical smog.
a.The energy required to split NO and O from NO2 is 305 KJ/mol. If there are 6.02E23 particles/mol, what is the energy required to do this? (I got 5.07E24)
b. What is the maximum wave length of radiation that could cause this dissociation?
c. Would this radiation be capable of producing the photoelectric effect in cesium metal (work function or binding energy = 3.05E-19 J/atom)? If so, what would be the kinetic energy of the emitted photoeletrons?
***I just need help with equations and a little bit on the process***
a. To find the energy required to split NO and O from NO2, we need to calculate the energy per particle.
Given:
- Energy to split NO and O from NO2 = 305 kJ/mol
- Number of particles per mole = 6.02E23 particles/mol
To find the energy per particle, we divide the total energy by the number of particles per mole:
Energy per particle = Energy to split NO and O from NO2 / Number of particles per mole
Energy per particle = 305 kJ/mol / 6.02E23 particles/mol
We can now calculate the answer:
Energy per particle ≈ 5.07E-19 kJ/particle
Since 1 kJ = 1000 J, we can convert this to joules:
Energy per particle ≈ 5.07E-22 J/particle
Now, if you multiply this value by the total number of particles, you will get the energy required to split NO and O from NO2:
Energy required = Energy per particle * Number of particles
Energy required ≈ 5.07E-22 J/particle * 6.02E23 particles ≈ 3.06 J
Therefore, the energy required to split NO and O from NO2 is approximately 3.06 J.
b. To find the maximum wavelength of radiation that could cause dissociation, we can use the equation:
Energy = (Planck's constant * speed of light) / wavelength
We know the energy required to split NO and O from NO2 is 3.06 J (from part a), so we can rearrange the equation to solve for wavelength:
wavelength = (Planck's constant * speed of light) / Energy
Planck's constant (h) ≈ 6.626E-34 J·s
Speed of light (c) ≈ 3.00E8 m/s
Substituting these values and the energy we found in part a:
wavelength = (6.626E-34 J·s * 3.00E8 m/s) / 3.06 J
After performing the calculation, you will find the maximum wavelength of radiation that could cause dissociation.
c. To determine if the radiation would be capable of producing the photoelectric effect in cesium metal, we need to compare the energy of the radiation to the work function or binding energy of cesium.
Given:
- Work function/binding energy of cesium = 3.05E-19 J/atom
If the energy of the radiation is equal to or greater than the work function, it would be capable of producing the photoelectric effect in cesium metal. To find the kinetic energy of the emitted photoelectrons, we can subtract the work function from the energy of the radiation:
Kinetic energy of emitted photoelectrons = Energy of radiation - Work function
After substituting the values and performing the calculation, you will find the kinetic energy of the emitted photoelectrons.