1) If an oxygen molecule had the energy required to dissociate, what could its v
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Question
1) If an oxygen molecule had the energy required to dissociate, what could its velocity be? What would its temperature be at this velocity? What wavelength of light could it emit? What color is this?
2) Why are two single atoms so much more reactive than O2?
3) Consider hydrogen energy level transitions:
a) calculate the energy to go from the first quantum level to the second
b) calculate the energy to go from the 10th quantum level to the 11th.
c) Make a general statement about the relative energy values of all the possible hydrogen electron transitions, the likelihood of the different transitions happening, and what you think the hydrogen emission spectrum would look like.
Explanation / Answer
O2 needs to be hit by an electron with energy 13.6 eV to ionise.
That's just the energy of an electron that's been accelerated from zero through a potential difference of 13.6 volts. (not much is it?). To actually do that, you just use a vacuum tube with 13.6 volts on the anode - easy.
If you want to convert that to velocity, you need to multiply by e which is 1.6 x 10-19. That gives you the kinetic energy in Joules.
Then use the mass of an electron (9.1 x 10-31) to get the velocity.
(use 1/2 mv2)
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