## 1B.9

Jacey Yang 1F
Posts: 101
Joined: Fri Aug 09, 2019 12:17 am

### 1B.9

A lamp rated at 32 W (1W = 1 J.s-1) emits violet light of wavelength 420 nm. How many photons of violet light can the lamp generate in 2.0 s? How many moles of photons are emitted in that time interval?

I'm not sure how to go about solving this problem. Can someone please explain?

Michelle Le 1J
Posts: 50
Joined: Fri Aug 09, 2019 12:16 am

### Re: 1B.9

Since they gave you the watts of the lamp, you would convert that to J/s and multiply that by 2 because of the 2 seconds in order to get the Joules. You would just need to find the energy of the photon emitted using E=hc/wavelength and then use that answer (which is in Joules/photon) and multiply that to the 64 J to find the number of photons generated. In order to find the moles, you would then proceed with Avogadro's number.

Ziyan Wang 3J
Posts: 51
Joined: Wed Sep 18, 2019 12:22 am

### Re: 1B.9

Energy per photon=h*c/lambda=6.63*10^-34*3.00*10^8/(420*10^-9)=4.74*10^-19
Total energy= 32*2=64
# of photons= Total energy/energy per photon=64/(4.74*10^-19)=1.35*10^20

Mariah
Posts: 104
Joined: Fri Aug 02, 2019 12:16 am

### Re: 1B.9

Can anyone explain how the units should turn out? Or how they work throughout the problem because I am having trouble with that.

ramiro_romero
Posts: 90
Joined: Sat Sep 07, 2019 12:16 am

### Re: 1B.9

To find photons, you first multiply Watts by 2 seconds and get 64 J/2sec as the Total Energy. Then, you find the energy per photon by using the formula E=(hc)/lambda, (energy per photon should be 4.717 x 10^-19). Divide energy per photon by total energy, and you get the number of photons [1.35 x 10^20 photons].

To find moles of photons, you divide the number of photons(1.35 x 10^20) by avogrados number (6.022 x 10^23), and get [2.25 x 10^-4 mol photons]

nshahwan 1L
Posts: 100
Joined: Fri Aug 30, 2019 12:18 am

### Re: 1B.9

I understand how to do this, but could someone explain why you divide the energy of the photon from the given watts?