A sample of gas occupies 100ml at 27 degree Celsius and 740mm pressure. The temperature the gas will have,when its volume is changed to 80ml at 740mm pressure is?

To find the temperature of the gas when its volume is changed to 80ml at constant pressure, we can use the combined gas law equation:

(P1 × V1) / T1 = (P2 × V2) / T2

where:
P1 = initial pressure of the gas
V1 = initial volume of the gas
T1 = initial temperature of the gas
P2 = final pressure of the gas
V2 = final volume of the gas
T2 = final temperature of the gas (what we want to find)

Given:
P1 = 740 mm
V1 = 100 ml
T1 = 27°C = 27 + 273 = 300 Kelvin
P2 = 740 mm (constant pressure)
V2 = 80 ml

Plugging in the given values into the equation, we get:

(740 × 100) / 300 = (740 × 80) / T2

Simplifying the equation:

74000 / 300 = 59200 / T2

Cross multiplying:

74000 × T2 = 300 × 59200

Dividing both sides by 74000:

T2 = (300 × 59200) / 74000

Calculating T2:

T2 = 240

Therefore, the temperature of the gas will be 240 Kelvin when its volume is changed to 80ml at constant pressure.

Only volume and temperatures change, pressure remains constant, Charles's law applies.

V1/T1=V2/T2

Temperatures must be converted to °K.
V1=100 ml
T1=27°C=300.15°K
V2=80 ml.

The above applies when the volume change is at constant pressure to avoid work done during reduction in volume.

240