Calculate energy emitted when electrons of 1.0 g of hydrogen undergo transition giving the spectral line of lowest energy in the visible region of its atomic spectra.

Question

Ramesh V · Answer

visible range wavelengths : 400 -750 nm

400nm corresponds to violet color band in visible region

Energy correspoding to it is : E = 1242 eV-nm /400 = 3.105 eV

1 gram hydrogen contains (1 mole of electrons) 6.022 x 10^23 electrons

1 electron volt = 1.602× 10^-19 joules

Total Energy = 1.602 * 10^-19 *6.022*10²³*3.105

= 299.55 KJ

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Calculate energy emitted when electrons of 1.0 g of hydrogen undergo transition giving the spectral line of lowest energy in the visible region of its atomic spectra.

Calculate energy emitted when electrons of 1.0 g of hydrogen undergo transition giving the spectral line of lowest energy in the visible region of its atomic spectra.

1 Answers

1 electron volt = 1.602× 10^-19 joules

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Calculate energy emitted when electrons of 1.0 g of hydrogen undergo transition giving the spectral line of lowest energy in the visible region of its atomic spectra.

Calculate energy emitted when electrons of 1.0 g of hydrogen undergo transition giving the spectral line of lowest energy in the visible region of its atomic spectra.

1 Answers

1 electron volt = 1.602× 10-19 joules

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1 electron volt = 1.602× 10^-19 joules