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. accuracy of the data matters alot more than its number of digits, organization or amount of detail. quantitative observation is more accepted than the qualitative observation.