A mixture of He
1 answer:
Answer : The partial pressure of nitrogen gas in the mixture is, 9.88 atm
Explanation :
According to the Dalton's Law, the total pressure of the gas is equal to the sum of the partial pressure of individual gases.
Formula used :
where,
= total pressure of gas = 13.6 atm
= partial pressure of helium gas = 1831 torr = 2.41 atm
= partial pressure of argon gas = 997 torr = 1.31 atm
Conversion used: (1 atm = 760 torr)
= partial pressure of nitrogen gas = ?
Now put all the given values in the above formula, we get:
Thus, the partial pressure of nitrogen gas in the mixture is, 9.88 atm
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P 15 atm
V₁ = 12x103 m3 -3 3 V₁ = 12x10 m" T₁ = 25°c T= 28815 K
P₁ = 1.52x10 Pa
Now, Finel quantities, T₂ = 35°C = 308.15 °K
V2= 851 = -3 3
Now
by ideal gas equation
P2Y2 T2
= PV, T2
1152 X106 x 12x16 3 x 308115 8,5×103 x 288,15 = Pa
=
21294×10 Pa
P₂ = 21264 Atm
final
pressure will be
21264 Adm.
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Answer:
Approximately (rounded to two significant figures.)
Explanation:
The unit of concentration is the same as
(moles per liter.) On the other hand, the volume of both the
solution and the original
solution here are in milliliters. Convert these two volumes to liters:
.
.
Calculate the number of moles of in that
of
solution:
.
reacts with
at a one-to-one ratio:
.
Coefficient ratio:
.
In other words, one mole of would neutralize exactly one mole of
. In this titration,
of
was required. Therefore, the same amount of
should be present in the original solution:
.
Calculate the concentration of the original solution:
.