The blue line of the hydrogen emission spectrum has a wavelength of 433.9 nm.

The blue line of the hydrogen emission spectrum has a wavelength of 433.9 nm.

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  1. 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  

  2. [tex]\large \boxed{4.578 \times 10^{-19} \text{ J}}[/tex]

    Explanation:

    The formula for the energy of a photon is

    E = hc/λ

    If λ = 433.9 nm, then  

    [tex]\begin{array}{rcl}E & = & \dfrac{6.626 \times 10^{-34} \text{ J$\cdot$s} \times 2.998 \times 10^{8}\text{ s}} {433.9 \times 10^{-9} \text{ m}}\\\\& = & 4.578 \times 10^{-19} \text{ J}\\\end{array}\\\text{The energy of one photon is $\large \boxed{\mathbf{4.578 \times 10^{-19}} \textbf{ J}}$}[/tex]

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