A sample of gas starts at 1.00 atm, 0.00 degrees Celsius, and 30.0 mL. What is the volume if the temperature increases to 27.0 degrees Celsius and the pressure increases to 2 atm?

16.48mL

Explanation:

The following data were obtained from the question:

Initial pressure (P1) = 1 atm

Initial temperature (T1) = 0°C = 0°C + 273 = 273K

Initial volume (V1) = 30mL

Final temperature (T2) = 27°C = 27°C + 273 = 300K

Final pressure (P2) = 2atm

Final volume (V2) =..?

Applying the general gas equation, the final volume of the gas can be obtained as follow:

P1V1/T1 = P2V2/T2

1 x 30/273 = 2 x V2/300

Cross multiply to express in linear form

273 x 2 x V2 = 30 x 300

Divide both side by 273 x 2

V2 = (30 x 300)/(273 x 2)

V2 = 16.48mL

Therefore, the new volume of the gas is 16.48mL

> b takes place in the gas phase in an isothermal tubular reactor. the feed is one mole of a per one mole of c, an inert. the entering temperature and pressure are 427°c and 10 atm, respectively. the gas constant r = 0.08206 atm · l/mol · k.