. A cylinder contains a mixture of N2 and O2 gases at a total pressure of 4.9 atm. The partial pressure of O2 is 0.7atm.Calculate the composition of O2 and N2 ?
Answers
Answer:
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Explanation:
Partial Pressure
Dalton’s Law of Partial Pressure
Dalton’s Law of Partial Pressure states the total pressure exerted by a mixture of gases is equal to the sum of the partial pressure of each individual gas.
LEARNING OBJECTIVES
Demonstrate an understanding of partial pressures and mole fractions.
KEY TAKEAWAYS
Key Points
The total pressure of a mixture of gases can be defined as the sum of the pressures of each individual gas:
P
t
o
t
a
l
=
P
1
+
P
2
+
…
+
P
n
.
The partial pressure of an individual gas is equal to the total pressure multiplied by the mole fraction of that gas.
Boyle’s Law and the Ideal Gas Law tell us the total pressure of a mixture depends solely on the number of moles of gas, and not the kinds of molecules; Dalton’s Law allows us to calculate the total pressure in a system from each gas’ individual contribution.
Key Terms
mole fraction: number of moles of one particular gas divided by the total moles of gas in the mixture
Dalton’s Law of Partial Pressures: the total pressure exerted by the mixture of non-reactive gases is equal to the sum of the partial pressures of each individual gas; also known as Dalton’s Law of Partial Pressures
Because it is dependent solely the number of particles and not the identity of the gas, the Ideal Gas Equation applies just as well to mixtures of gases is does to pure gases. In fact, it was with a gas mixture—ordinary air—that Boyle, Gay-Lussac, and Charles performed their early experiments. The only new concept we need to deal with gas mixtures is partial pressure, a concept invented by the famous English chemist John Dalton (1766-1844). Dalton correctly reasoned that the low density and high compressibility of gases were indicative of the fact that they consisted mostly of empty space; from this, it Dalton concluded that when two or more different gases occupy the same volume, they behave entirely independently of one another.
Dalton’s Law (also called Dalton’s Law of Partial Pressures) states that the total pressure exerted by the mixture of non-reactive gases is equal to the sum of the partial pressures of individual gases. Mathematically, this can be stated as follows:
P
t
o
t
a
l
=
P
1
+
P
2
+
…
+
P
n
where P1, P2 and Pn represent the partial pressures of each compound. It is assumed that the gases do not react with each other.
EXAMPLE
A 2.0 L container is pressurized with 0.25 atm of oxygen gas and 0.60 atm of nitrogen gas. What is the total pressure inside the container?
P
t
o
t
a
l
=
P
O
2
+
P
N
2
=
0.25
+
0.60
=
0.85
atm
The total pressure inside the contain is 0.85 atm.
Answer:
Explanation:w
N
2
=7 g,w
Ar
=8 g
n
N
2
=7/28=0.25 mole,n
Ar
=8/40=0.20 mole
X
N
2
=
0.25+0.20
0.25
=
9
5
P
N
2
=X
N
2
×P
Total
=
9
5
×27=15 bar