The soulustion. turn cloudy due to the precipitation of Sulphur.
Answer:
B) Their valence shell is full
Explanation:
In order to be classified as a noble gas, an element must have a complete octet/ a full shell of valence electrons, as shown in answer B.
A and C are just incorrect. Since noble gasses are very unstable, D is a true statement, but is isn't the correct answer as this does not explain why they are inert.
<h3>Hope this was helpful!</h3>
Explanation:
substance Q could be <em><u>oxygen (O2)</u></em>
substance R could be <em><u>carbon</u></em><em><u> </u></em><em><u>d</u></em><em><u>i</u></em><em><u>o</u></em><em><u>x</u></em><em><u>i</u></em><em><u>d</u></em><em><u>e</u></em><em><u> </u></em><em><u>(</u></em><em><u>C</u></em><em><u>O</u></em><em><u>2</u></em><em><u>)</u></em>
Answer:
Meteorologists look at data help from the computer about temperature, pressure, humidity, and wind speed, among many other data points to try and accurately predict the weather.
Answer:
Ammonia is the richest source of nitrogen on a mass percentage basis because it has 82.35% of nitrogen by mass.
Explanation:
Percentage of element in compound :
![=\frac{\text{number of atoms}\times text{Atomic mass}}{\text{molar mas of compound}}\times 100](https://tex.z-dn.net/?f=%3D%5Cfrac%7B%5Ctext%7Bnumber%20of%20atoms%7D%5Ctimes%20text%7BAtomic%20mass%7D%7D%7B%5Ctext%7Bmolar%20mas%20of%20compound%7D%7D%5Ctimes%20100)
(a) Urea, ![(NH_2)_2CO](https://tex.z-dn.net/?f=%28NH_2%29_2CO)
Molar mass of urea = 60 g/mol
Atomic mass of nitrogen = 14 g/mol
Number of nitrogen atoms = 2
![N\%=\frac{2\times 14 g/mol}{60 g/mol}\times 100=46.67\%](https://tex.z-dn.net/?f=N%5C%25%3D%5Cfrac%7B2%5Ctimes%2014%20g%2Fmol%7D%7B60%20g%2Fmol%7D%5Ctimes%20100%3D46.67%5C%25)
(b) Ammonium nitrate, ![NH_4NO_3](https://tex.z-dn.net/?f=NH_4NO_3)
Molar mass of ammonium nitrate = 80 g/mol
Atomic mass of nitrogen = 14 g/mol
Number of nitrogen atoms = 2
![N\%=\frac{2\times 14 g/mol}{80 g/mol}\times 100=35.00\%](https://tex.z-dn.net/?f=N%5C%25%3D%5Cfrac%7B2%5Ctimes%2014%20g%2Fmol%7D%7B80%20g%2Fmol%7D%5Ctimes%20100%3D35.00%5C%25)
(c) Nitric oxide, NO
Molar mass of nitric oxide = 30 g/mol
Atomic mass of nitrogen = 14 g/mol
Number of nitrogen atoms = 1
![N\%=\frac{1\times 14 g/mol}{30 g/mol}\times 100=46.67\%](https://tex.z-dn.net/?f=N%5C%25%3D%5Cfrac%7B1%5Ctimes%2014%20g%2Fmol%7D%7B30%20g%2Fmol%7D%5Ctimes%20100%3D46.67%5C%25)
(d) Ammonia, ![NH_3](https://tex.z-dn.net/?f=NH_3)
Molar mass of ammona = 17 g/mol
Atomic mass of nitrogen = 14 g/mol
Number of nitrogen atoms = 1
Ammonia is the richest source of nitrogen on a mass percentage basis because it has 82.35% of nitrogen by mass.