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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.
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 -- Please feel free to post as many doubts on our disucssion forum as you can. If you find any question difficult to understand - post it here and we will get you the answer and detailed solution very quickly.We are all IITians and here to help you in your IIT JEE preparation. All the best. Regards, Naga Ramesh IIT Kgp - 2005 batch
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
Total Energy = 1.602 * 10-19 *6.022*1023*3.105
= 299.55 KJ
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Please feel free to post as many doubts on our disucssion forum as you can. If you find any question difficult to understand - post it here and we will get you the answer and detailed solution very quickly.We are all IITians and here to help you in your IIT JEE preparation. All the best. Regards, Naga Ramesh IIT Kgp - 2005 batch
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