solution;
standard value of g on earth = 9.80665
value derived from experiment = 10.06
error in reading the value = 10.06 - 9.80665
= 0.25335
% error ![= \frac{0.25335}{9.80665\times100}](https://tex.z-dn.net/?f=%3D%20%5Cfrac%7B0.25335%7D%7B9.80665%5Ctimes100%7D)
= 2.583 %
Most ionic compounds fall in the category of chemicals called salts. ... Electrolytes, or in other words compounds that are ionizable in solution, play an essential role in many body functions. Cells create electrical energy as ions move from the solutions inside the cells of our body<span> to the solutions outside the cells.
I hope my answer has come to your help. God bless and have a nice day ahead!
</span>
Answer:
The wavelength of the light emitted by a hydrogen atom for the given transition is 2166 nm.
Explanation:
The energy of nth energy levels of the H atom is given as:
![E_n = -2.18 \times 10^{-18} \times \frac{1}{n^2} J](https://tex.z-dn.net/?f=E_n%20%3D%20-2.18%20%5Ctimes%2010%5E%7B-18%7D%20%5Ctimes%20%5Cfrac%7B1%7D%7Bn%5E2%7D%20J)
Energy of the seventh energy level = ![E_7](https://tex.z-dn.net/?f=E_7)
![E_7=-2.18 \times 10^{-18} \times \frac{1}{7^2} J](https://tex.z-dn.net/?f=E_7%3D-2.18%20%5Ctimes%2010%5E%7B-18%7D%20%5Ctimes%20%5Cfrac%7B1%7D%7B7%5E2%7D%20J)
![E_7=-2.18 \times 10^{-18} \times \frac{1}{7^2} J=-4.4490\times 10^{-20} J](https://tex.z-dn.net/?f=E_7%3D-2.18%20%5Ctimes%2010%5E%7B-18%7D%20%5Ctimes%20%5Cfrac%7B1%7D%7B7%5E2%7D%20J%3D-4.4490%5Ctimes%2010%5E%7B-20%7D%20J)
Energy of the seventh energy level = ![E_4](https://tex.z-dn.net/?f=E_4)
![E_4=-2.18 \times 10^{-18} \times \frac{1}{4^2} J](https://tex.z-dn.net/?f=E_4%3D-2.18%20%5Ctimes%2010%5E%7B-18%7D%20%5Ctimes%20%5Cfrac%7B1%7D%7B4%5E2%7D%20J)
![E_4=-2.18 \times 10^{-18} \times \frac{1}{16} J=-1.3625\times 10^{-19} J](https://tex.z-dn.net/?f=E_4%3D-2.18%20%5Ctimes%2010%5E%7B-18%7D%20%5Ctimes%20%5Cfrac%7B1%7D%7B16%7D%20J%3D-1.3625%5Ctimes%2010%5E%7B-19%7D%20J)
Energy of the light emitted will be equal to the energy difference of the both levels.
![E=E_7-E_4=-4.4490\times 10^{-20} J-(-1.3625\times 10^{-19} J)](https://tex.z-dn.net/?f=E%3DE_7-E_4%3D-4.4490%5Ctimes%2010%5E%7B-20%7D%20J-%28-1.3625%5Ctimes%2010%5E%7B-19%7D%20J%29)
![E=9.176\times 10^{-20} J](https://tex.z-dn.net/?f=E%3D9.176%5Ctimes%2010%5E%7B-20%7D%20J)
Wavelength corresponding to energy E can be calculated by using Planck's equation:
![E=\frac{hc}{\lambda }](https://tex.z-dn.net/?f=E%3D%5Cfrac%7Bhc%7D%7B%5Clambda%20%7D)
![\lambda =\frac{hc}{E}=\frac{6.626\times 10^{-34} Js\times 3\times 10^8 m/s}{9.176\times 10^{-20} J}=2.166\times 10^{-6} m=2166 nm](https://tex.z-dn.net/?f=%5Clambda%20%3D%5Cfrac%7Bhc%7D%7BE%7D%3D%5Cfrac%7B6.626%5Ctimes%2010%5E%7B-34%7D%20Js%5Ctimes%203%5Ctimes%2010%5E8%20m%2Fs%7D%7B9.176%5Ctimes%2010%5E%7B-20%7D%20%20J%7D%3D2.166%5Ctimes%2010%5E%7B-6%7D%20m%3D2166%20nm)
The wavelength of the light emitted by a hydrogen atom for the given transition is 2166 nm.
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