Consider two 5 L chambers. In one, there are 5.00 g O₂, and in the other there are 5.00 g He. Which has the higher pressure at r
1 answer:
Answer:
He have higher pressure at room temperature.
Explanation:
It is given that both the gases are kept in 5 L chambers.
Therefore, volume is constant.
Also, they both are at room temperature, so temperature is also constant.
Now, number of moles of =
Also, number of moles of He =
Now, according to GAS LAW,
( all terms have their usual meaning).
In this case, V, R and T are constant.
So, pressure is directly proportional to n i.e number of moles.
So, moles of He is more than moles of .
Therefore, He have higher pressure at room temperature.
Hence , this is the required solution.
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Answer:
a. the maximum number of σ bonds that the atom can form is 4
b. the maximum number of p-p bonds that the atom can form is 2
Explanation:
Hybridization is the mixing of at least two nonequivalent orbitals, in this case, we have the mixing of one <em>s, 3 p </em> and <em> 2 d </em> orbitals. In hybridization the number of hybrid orbitals generated is equal to the number of pure atomic orbital, so we have 6 hybrid orbital.
The shape of this hybrid orbital is octahedral (look the attached image) , it has 4 orbital located in the plane and 2 orbital perpendicular to it.
This shape allows the formation of maximum 4 σ bond, because σ bonds are formed by orbitals overlapping end to end.
And maximum 2 p-p bonds, because p-p bonds are formed by sideways overlapping orbitals. The atom can form one with each one of the orbitals located perpendicular to the plane.
