A 1.20 g sample of water is injected into an evacuated 5.00 l flask at 65°c. part of the water vaporizes and creates a pressure
1 answer:
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Answer:
Explanation:
From the given information:
The density of O₂ gas =
here:
P = pressure of the O₂ gas = 310 bar
=
= 305.97 atm
The temperature T = 415 K
The rate R = 0.0821 L.atm/mol.K
molar mass of O₂ gas = 32 g/mol
∴
= 287.37 g/L
To find the density using the Van der Waal equation
Recall that:
the Van der Waal constant for O₂ is:
a = 1.382 bar. L²/mol² &
b = 0.0319 L/mol
The initial step is to determine the volume = Vm
The Van der Waal equation can be represented as:
where;
R = gas constant (in bar) = 8.314 × 10⁻² L.bar/ K.mol
Replacing our values into the above equation, we have:
After solving;
V = 0.1152 L
∴
= 277.77 g/L
We say that the repulsive part of the interaction potential dominates because the results showcase that the density of the Van der Waals is lesser than the density of ideal gas.
The question is incomplete. Here is the complete question.
Aqueous solutions of and
, 0.10 M each, are combined. A white precipitate is observed in the container after mixing. he precipitate is filtered andcarefully rinsed with distilled water to remove other ions. A sample of the precipitate is added to 100 mL of 0.1 M NaCl. A second sample of the precipitate is then added to 100 mL of 0.1 M HCl. What would be observed in each case?
Observation upon Observation upon
addition of precipitate addition of precipitate
to NaCl(aq) to HCl(aq)
(A) additional precipitates forms no visible reaction occurs
(B) no visible reaction occurs gas is produced and some precipitate dissolves
(C) no visible reaction occurs no visible reaction occurs
(D) additional precipitates forms gas is produced and some
precipitate dissolves
Answer: (B) No visible reaction occurs; Gas is produced and some precipitate dissolves
Explanation: When aqueous solutions of and
are combined, it reacts according to the following balanced equation:
→
forming calcium carbonate (), which, as it is insoluble in water, precipitates as a solid of the color white. This process is <u>Precipitation</u> and this reaction is a <u>Precipitation</u> <u>Reaction</u>.
When calcium carbonate reacts with NaCl it produces:
→
Now, calcium chloride is an inorganic compound very soluble in water, so, in this reaction, there are no precipitate and <u>no visible reaction occurs</u>.
When reacts with hydrochloridric acid, the balanced reaction is
→
which, also produces calcium chloride and carbonic acid.
Both are soluble in water but, when carbonic acid is in an "aqueous state", carbonic acid, it dissociates, forming carbon dioxide and water. Therefore, <u>gas is produced and some precipitate dissolves</u>.
In conclusion, sentence B is the correct alternative.