Question

A gas 'X' at 15°C is heated until its pressure doubles and volume triples from the original pressure and volume. If the original volume is 1000 cc., calculate the temperature to which it should be heated. ​

Answer 1

A gas 'X' at 15°C is heated until its pressure doubles and volume triples from the original pressure and volume. If the original volume is 1000 cc., it should be heated to 1455.75°C

We have given gas X

Assuming the Gas to be ideal gas .

Initial temperature of gas in °C =15°C

• Converting temperature in Kelvin =273.15 +15

=288.15K

Let

• Initial Pressure of gas = P
• nitial Pressure of gas = P Initial volume of gas =V

According to Ideal gas equation

$pv = nrt$

• Here n=no of moles & R=gas constant both are constant in above question.
• Given the final volume is triple of initial so

Final volume =3V

• Final pressure of gas is double of initial pressure

Final pressure =2P

We have to find out Final temperature

So if nR is constant then

$\frac{p1v1}{t1} = \frac{p2v2}{t2}$

$\frac{pv}{288.15} = \frac{2p \times 3v}{t2}$

• From above equation

t2 =288.15×6

$t2 = 288.15 \times 6 = 1728.90$

• Final temperature is =1728.90K
• Final temperature in °C=1728.90-273.15
• Final temperature of the gas will be 1455.75°C

Answer 2

Step-by-step explanation:

Temperature of heating = 6(273 + 15) = 1728 K

= 1455°C