Question

A gas cylinder is filled with gas occupies 150cc at 200C and 800mm of Hg
pressure. What will be its volume at 270C and 300mm of Hg pressure?

Answer 1

Explanation:

PHYSICS

At 0

∘

and 760mm Hg pressure, a gas occupies a volume of 100cm

3

. Kelvin temperature of the gas is increased by one-fifth and the pressure is increased one and a half times. Calculate the final volume of the gas

HARD

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ANSWER

GivenT

1

=0

0

=273KandP

1

=760mmofHg

T

2

=273+

5

273

=327.6KandP

2

=760+

2

760

=1140mmofHg

ASperidealgasequation

PV=nRTasinboththecasesgasissamethan,

T

1

P

1

V

1

=

T

2

P

2

V

2

V

2

=

273×1140

327.6×760×100

=80cm

3

hope you got it

Answer 2

Answer:

Volume of the gas = 0.43 L

Explanation:

$\Large{\underline{\sf{Given:}}}$

• Volume of the gas (V₁) = 150 cc
• Temperature of the gas (T₂) = 200° C
• Pressure (P₁) = 800 mm of Hg
• Temperature (T₂) = 270° C
• Pressure (P₂) = 300 mm of Hg

$\Large{\underline{\sf{To\:Find:}}}$

• Volume of the gas (V₂)

$\Large{\underline{\sf{Solution:}}}$

➠ First we have to covert all the given datas to the respective S.I units.

➠ Pressure:

    800 mm of Hg = 1 atm

    300 mm of Hg = 0.4 atm

➠ Temperature:

     200° C = 473.15 K

     270° C = 543.15 K

➠ Volume:

    150 cc = 0.15 L

➠ Now by the Ideal gas equation we know that,

    $\tt{\dfrac{P_1V_1}{T_1} =\dfrac{P_2V_2}{T_2} }$

➠ Substitute the data,

    $\tt{\dfrac{1\times 0.15}{473.15} =\dfrac{0.4\:V_2}{543.15} }$

➠ Simplifying,

     3.17 × 10⁻⁴ = 7.36 × 10⁻⁴ × V₂

     V₂ = 3.17/7.36

     V₂ = 0.43 L

➠ Hence the gas occupies a volume of 0.43 L.

    $\boxed{\bold{Volume\:of\:the\:gas=0.43\:L}}$