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.
Transportation seems like the right answer
Answer:
0.4
The efficiency is defined as the work done divided by the heat provided at Th. ε = W/Qh = 400 J/1000 J = 0.4 The Carnot efficiency is given in terms of the high and low temperatures.
Hope this helps, please let me know if it is wrong.
Answer:
If the substance is a liquid or solid, production of an odor would indicate a chemical change.
Explanation:
Answer:
6.69 moles
Explanation:
Data obtained from the question include:
Volume = 2230mL
Molarity of NaOH = 3 M
First, we'll convert 2230mL to L. This is illustrated below:
1000mL = 1L
2230mL = 2230/1000 = 2.23L
Now, we can obtain the number of mole of NaOH in the solution as follow:
Molarity = mole /Volume
Mole = Molarity x Volume
Mole of NaOH = 3 x 2.23
Mole of NaOH = 6.69 moles
Therefore, the total number of mole of the solute (NaOH) in the solution is 6.69 moles