Answer:
The pressure of H₂(g) = 741 torr
Explanation:
Given that:
The atmospheric pressure measured in the lab = 765 torr
The vapor pressure of water = 24 torr
By applying Dalton's Law of Partial Pressure :
Making The Pressure inside the tube due to the H₂(g) the subject of the formula :
we have:
= (765 -24) torr
= 741 torr
Answer:
NO = 0.0265 mol
Br₂ = 0.0133 mol
NOBr = 0.0389 mol
Explanation:
Let's consider the following reaction.
2 NO(g) + Br₂(g) ⇄ 2 NOBr(g)
We can find the composition at equilibrium using an ICE chart. Let x be an unknow amount.
2 NO(g) + Br₂(g) ⇄ 2 NOBr(g)
I 0.0655 0.0328 0
C -2x -x +2x
E 0.0655 - 2x 0.0328 - x 2x
At equilibrium, the mixture contains 0.0389 mol NOBr. Then,
0.0389 mol = 2x
x = 0.0195 mol
The composition of the equilibrium mixture is:
NO = 0.0655 - 2x = 0.0265 mol
Br₂ = 0.0328 - x = 0.0133 mol
NOBr = 0.0389 mol
As known, nitrogen could form 3 bonds based on octet rule, because it has 5 valence electrons. That means it needs 3
Answer: The pH of the solution is 5.65
Explanation:
The relationship between the pH and the pOH is that .
Given this, we can plug in the pOH and subtract that from 14.
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