A sample of gas starts at 1.2 atm, 107 degrees C° and 1,540 mL what is the volume in mL if the temps true increases to 110 C° and the pressure increases to 3.6 atm?

517ml

Explanation:

Given that:

Volume of gas V1 = 1540mL

Temperature T1 = 107°C

Convert Celsius to Kelvin

(107°C + 273 = 380K)

Initial Pressure P1 = 1.2 atm

Final Volume V2 = ?

Final temperature T2 = 110°C

(110°C + 273 = 383K)

Final pressure = 3.6 atm

Then, apply the general gas equation

(P1V1)/T1 = (P2V2)/T2

(1.2 x 1540)/380 = (3.6 x V2)/383

1848/380 = 3.6V2/383

4.86 = 0.0094V2

Divide both sides by 0.0094

4.86/0.0094 = 0.0094V2/0.0094

517 = V2

Thus, the final volume is 517ml