A sample of gas occupies 40.0 mL at - 123°C. What volume does the sample occupy at 27°C if the pressure is held constant? V1T2 = V2T1 Don't forget to convert temperature to kelvin! Group of answer choices 8.80 mL 20.0 mL 80. ML 182 mL

80mL

Explanation:

Step 1:

Data obtained from the question.

Initial Volume (V1) = 40mL

Initial temperature (T1) = - 123°C

Final temperature (T2) = 27°C

Final volume (V2) = ... ?

Step 2:

Conversion of celsius temperature to Kelvin temperature.

T (K) = T (°C) + 273

Initial temperature (T1) = - 123°C =

-123°C + 273 = 150K

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

Step 3:

Determination of the final volume.

This can be obtained as follow:

V1/T1 = V2/T2

Initial Volume (V1) = 40mL

Initial temperature (T1) = 150K

Final temperature (T2) = 300

Final volume (V2) = ... ?

V1/T1 = V2 / T2

40/150 = V2 / 300

Cross multiply

150 x V2 = 40 x 300

Divide both side by 150

V2 = (40 x 300) / 150

V2 = 80mL

Therefore, the new volume of the gas is 80mL