A container having 11g CO2 , 42g CO , 6.4g SO2 . If all oxygen is removed and kept in another container . Calculate the volume of O2 gas ???
Answers
Answer:
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Explanation:
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Answer:
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Explanation:
A tank contains a mixture of 54.5 g of oxygen gas and 68.9 g of carbon dioxide gas at 38°C. The total pressure in the tank is 10.00 atm. How do you calculate the partial pressure (in atm) of each gas in the mixture?
You can solve this problem by using Dalton's Law of Partial Pressures, which states that the partial pressure of a component of a gaseous mixture depends on the mole ratio of said component and the total pressure of the gaseous mixture.
∣
∣
∣
∣
¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯
a
a
P
i
=
χ
i
×
P
total
a
a
∣
∣
−−−−−−−−−−−−−−−−−−
, where
P
i
- the partial pressure of component
i
χ
i
- its mole fraction in the mixture
P
total
- the total pressure of the mixture
Since you already know the total pressure of the mixture, focus on finding how many moles of each gas you get in the mixture.
To do that, use the molar masses of the two gases. You will have
54.5
g
⋅
1 mole O
2
32.0
g
=
1.703 moles O
2
68.9
g
⋅
1 mol CO
2
44.01
g
=
1.566 moles CO
2
The total number of moles present in the mixture will be
n
total
=
n
O
2
+
n
C
O
2
n
total
=
1.703 moles
+
1.566 moles
=
3.269 moles