Answer:
3.6667
Explanation:
<u>For helium gas:</u>
Using Boyle's law
Given ,
V₁ = 3.0 L
V₂ = 9.0 L
P₁ = 5.6 atm
P₂ = ?
Using above equation as:
<u>The pressure exerted by the helium gas in 9.0 L flask is 1.8667 atm</u>
<u>For Neon gas:</u>
Using Boyle's law
Given ,
V₁ = 4.5 L
V₂ = 9.0 L
P₁ = 3.6 atm
P₂ = ?
Using above equation as:
<u>The pressure exerted by the neon gas in 9.0 L flask is 1.8 atm</u>
<u>Thus total pressure = 1.8667 + 1.8 atm = 3.6667 atm.</u>
Answer:
Straight connection
Explanation:
All synthetic items are made in a chemistry lab.
Natural - Organic
Chemical/Synthetic - Inorganic
Answer:
![AU^{3+} : [Rn] 5f^3](https://tex.z-dn.net/?f=AU%5E%7B3%2B%7D%20%3A%20%5BRn%5D%205f%5E3)
Explanation:
Writing electronic configuration of any element you should know atomic number of that element ,
and also electrons are filling according to their energy level and first electron is filled in the lower energy orbital
and it follows n+1 rule if n+1 is same for two orbital electron will go first in the lowest value of n.
writing electronic configuration of ion can be done like first for their neutral atom and then add or remove electron it will make things easy because there are also some eception case their you may do wrong.
![AU : [Rn] 5f^3 6d^1 7s^2](https://tex.z-dn.net/?f=AU%20%3A%20%5BRn%5D%205f%5E3%206d%5E1%207s%5E2)
remove three electron from outer most shell of AU
![AU^{3+} : [Rn] 5f^3](https://tex.z-dn.net/?f=AU%5E%7B3%2B%7D%20%3A%20%5BRn%5D%205f%5E3)
The ideal gas law is the generalized gas equation that depicts the state of the hypothetical gas condition. Moles of oxygen take in is 2.42 mol.
<h3>What is the Ideal gas equation?</h3>
The ideal gas equation gives the equation about the product of the pressure and the volume to be equal to that of the product of moles, temperature and the gas constant of the gas.
The formula for the ideal gas equation is:
![\rm PV = nRT](https://tex.z-dn.net/?f=%5Crm%20PV%20%3D%20nRT)
Where,
- Pressure (P) = 1000 kPa
- Volume (V) = 6.0 L
- Ideal gas constant (R) =
![8. 31 \;\text{LkPa/mol K}](https://tex.z-dn.net/?f=8.%2031%20%5C%3B%5Ctext%7BLkPa%2Fmol%20K%7D)
- Temperature (T) = 298 K
- Number of moles = n
Substituting values in the equation:
![\begin{aligned} 1000 \times 6 &= \rm n \times 8.31 \times 298\\\\\rm n &= \dfrac{1000 \times 6}{8.31 \times 298}\\\\& = 2.42\;\rm moles\end{aligned}](https://tex.z-dn.net/?f=%5Cbegin%7Baligned%7D%201000%20%5Ctimes%206%20%26%3D%20%5Crm%20n%20%5Ctimes%208.31%20%5Ctimes%20298%5C%5C%5C%5C%5Crm%20n%20%26%3D%20%5Cdfrac%7B1000%20%5Ctimes%206%7D%7B8.31%20%5Ctimes%20298%7D%5C%5C%5C%5C%26%20%3D%202.42%5C%3B%5Crm%20moles%5Cend%7Baligned%7D)
Therefore, 2.42 moles of oxygen is taken in during the respiration process.
Learn more about the ideal gas equation here:
brainly.com/question/3624088