A certain volume of a gas is under a pressure of 1800 mm of Hg. When the
pressure is increased by 20%, the gas occupies 2700 ml. If this change occurs at
a constant temperature, calculate the initial volume of the gas
wanted written answer
Answers
Answer:
GIVEN :-
A gas of certain volume is under a pressure of 900 mm of Hg
The volume occupied by the gas when the pressure was increased by 300 mm of Hg is 2700 ml
TO FIND :-
The volume occupied by the gas initially
SOLUTION :-
In the same way ,
Final pressure is increased by 300 mm of Hg = 900 mm of Hg + 300 mm of Hg = 1200 mm of Hg
We have ,
P₁ = 1.18 atm , P₂ = 1.57 atm
V₁ = ? , V₂ = 2700 ml = 2.7 litres
According to Boyle's law ,
∴ The volume occupied by the gas initially is 3.6 litres or 3.59 litres
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Answer:
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A gas occupies one litre under atomospheric pressure. What will be the volume of the same amount of gas under 750 mm of Hg the temperature ?
Medium
Solution
verified
Verified by Toppr
Given
V
1
=1 litre
P
1
=1 atm
V
2
=?
P
2
=
760
750
atm (at same T)
∵(1 atm=760mm)
P
1
V
1
=P
2
V
2
1×1=
760
750
×V
2
v
2
=
750
760
v
2
=1.0133 litre
=1013.3 mL
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