Question

A gas occupy 400 ml volume at 47 °C and 800 mm of Hg pressure. What will be its
pressure at a height where the temperature is 27 °C and volume of the gas is 450 ml ?
​

Answer 1

Answer:

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>>At 25^oC and 760 mm of Hg pressure, a ga

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At 25

o

C and 760 mm of Hg pressure, a gas occupies 600 mL volume. What will be its pressure at a height where temperatures is 10

o

C and volume of the gas is 640 mL?

Medium

Solution

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Correct option is A)

Given, P

1

=760mmHg, V

1

=600mL

T

1

=273+25=298K

P

2

=?

V

2

=640mL and T

2

=273+10=283K

According to combined gas law equation,

T

1

P

1

V

1

=

T

2

P

2

V

2

or P

2

=

V

2

T

1

P

1

V

1

T

2

=

(640mL)(298K)

(760mmHg)×(600mL)×(283K)

= 676.6mmHg

Answer 2

Answer:

The pressure is 666.67mmHg.

Explanation:

From ideal gas it can be derived

                                   $P1V1/T1=P2V2/T2$

           ∴                           $P2=P1V1/T1*T2/V2$

V1=400ml

T1= 47°c ⇒320K

P1=800mmHg

P2=?

T2=27°c

V2=450ml

∴ P2= 800*400*300/320*450

       =666.67mmHg

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