A given mass of a gas occupies 572 cm3 at 13 degree Celsius and 725 mm Hg pressure. What will be its volume at 24 degree celcius and 792 mm Hg pressure?
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Answer:
Volume = 966.66666 cm³
Explanation:
From all the gas laws we get,
PV = nRT
P = \dfrac{nRT}{V}
V
nRT
Therefore,
P ∝ \dfrac{T}{V}
V
T
or
\dfrac{PV}{T}
T
PV
= constant
Using the above eqution we get,
\dfrac{P_1V_1}{T_1}= \dfrac{P_2V_2}{T_2}
T
1
P
1
V
1
=
T
2
P
2
V
2
From the question we get,
P₁ = 725 mm Hg P₂ = 792 mm Hg
V₁ = 572 cm³ V₂ = ?
T₁ = 130° C T₂ = 240° C
Substituting all theses values we get,
\dfrac{725 \times 572}{130} =\dfrac{792 \times V_2}{240}
130
725×572
=
240
792×V
2
\dfrac{725 \times 572 \times 240}{130 \times 792} =V_2
130×792
725×572×240
=V
2
V_2 = 966. \bar6V
2
=966.
6
ˉ
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