The blue line of the hydrogen emission spectrum has a wavelength of 433.9 nm. a hydrogen emission spectrum has a violet, a blue, a teal, and a red line. calculate the energy of one photon of this light.

The energy of one photon of this light is 4.568 × 10∧ -19 J  

Explanation:

Given data:

wavelength = 433.9 nm or 433.9 × 10∧-9 m

The value of speed of light is 3× 10∧8 m/s and plancks constant is 6.626 × 10∧-34 m²Kg/s

Formula:

E= hc/λ

E= energy of photon

h= plancks constant

c= speed of light

λ= wavelength of given light

Solution:

E= hc / λ

E = 6.626 × 10∧-34 m²Kg/s × 3× 10∧8 m/s / 433.9 × 10∧-9 m

E = 19.878 × 10∧-26 m²Kg/s² / 433.9 × 10∧-9 m

E = 0.04568 × 10∧ -17 J            (Kg m²/s² =J)

E = 4.568 × 10∧ -19 J  

Explanation:

The formula for the energy of a photon is

E = hc/λ

If λ = 433.9 nm, then  

when [oh-] is 10-5  m, and [h3o+] is 10-9  m, the poh is 5 and ph is 9. again in both cases the sum of ph and poh is 14. however, the hydrogen ion concentration is not always going to be equal to exactly 1 x 10 raised to a negative number. for example, we skipped over the value of 2.0 x 10-7.