I'm working on homework and the computer won't accept my answer.
Calculate the energy of photons with wavelenth 0.174 nm.
I used the equation E=hv and got the answer to be 1.14 X 10^-17. It says i'm off by a multiple of ten. I have no idea where I messed up.
Are you using frequency instead of wavelength?
E = hc/wavelength
h = 6.626 x 10^-34 J*sec
c = 3 x 10^8 m/s
wavelength = 0.174 x 10^-9 meters.
I find 1.14 x 10^-15 joules so I think you are off by 100.
(a) Calculate the energy of photons of wavelength 3.1 µm.
To calculate the energy of photons, you can use the equation E = hc/λ, where E represents the energy, h is the Planck's constant (6.626 x 10^-34 J*s), c is the speed of light (3.00 x 10^8 m/s), and λ is the wavelength in meters.
In this case, you have a wavelength of 0.174 nm. However, you need to convert it to meters to use it in the equation.
1 nm = 1 x 10^-9 m
Therefore, 0.174 nm = 0.174 x 10^-9 m
Now substitute the values into the equation:
E = (6.626 x 10^-34 J*s * 3.00 x 10^8 m/s) / (0.174 x 10^-9 m)
Perform the calculation:
E = (1.9888 x 10^-25 J*m) / (0.174 x 10^-9 m)
E ≈ 1.14 x 10^-16 J
Based on your answer, it appears that you multiplied the numerator correctly but made a mistake in the denominator. Check your calculation and make sure you use the correct value for the wavelength. Note that the final answer is 1.14 x 10^-16 J, not 1.14 x 10^-17 J as you initially calculated.
Remember to double-check your calculations and units to ensure accuracy.