Question

600.0 ML sample of nitrogen is warmed from 77.0°C to 86.0°C find its new volume if the pressure remains constant

Answer 1

Given :

➳ Initial volume = 600ml

➳ Initial temperature = 77°C

➳ Final temperature = 86°C

➳ Pressure remains constant.

To Find :

➨ Final volume of nitrogen gas.

Conversion :

➠ 0°C = 273K

➠ 77°C = 77 + 273 = 350K

➠ 86°C = 86 + 273 = 359K

SoluTion :

⇒ As per charle's law, Pressure remaining constant, the volume of a fixed mass of a gas is directly proportional to its absolute temperature.

$\longrightarrow\tt\:V\propto T\:(at\:constant\:P)\\ \\ \longrightarrow\tt\:\dfrac{V_1}{T_1}=\dfrac{V_2}{T_2}\\ \\ \longrightarrow\tt\:\dfrac{600}{350}=\dfrac{V_2}{359}\\ \\ \longrightarrow\tt\:V_2=\dfrac{600\times 359}{350}\\ \\ \longrightarrow\underline{\boxed{\bf{V_2=615.42\:ml}}}$

Answer 2

★Answer★

“Charles Law:”

»Charles law also sometimes referred to as the law of volumes gives a detailed account of how gas expands when the temperature is increased. Conversely, when there is a decrease in temperature it will lead to a decrease in volume.

When we compare a substance under two different conditions, from the above statement we can write this in the following manner:

»V2/V1=T2/T1

OR

»V1/T2=V2/T1

This above equation depicts that as absolute temperature increases, the volume of the gas also goes up in proportion.

In other words, Charle’s law is a special case of the ideal gas law. The law is applicable to the ideal gases that are held at constant pressure but the temperature and volume keep changing.

★Solution★

V1=600mL

T1=77°C=350.15°k

T2=86°C=359.15°K

V2=?

NOW,

600/350=V2/359

V2=359(12/7)

V2=359×12/7

V2=4308/7

V2=615mL

therefore,

V2=615mL