During laparoscopic surgery, CO2 gas is used to expand the abdomen to help create a larger working space. If the CO2 injected into the abdomen produces a pressure of 20.0 mmHg
and a volume of 4.00 L at 32.0C, how many grams of CO2 were used?

The answer to your question is     V2 = 4.97 l

Explanation:

Data

Volume 1 = V1 = 4.40 L                    Volume 2 =

Temperature 1 = T1 = 19°C               Temperature 2 = T2 = 37°C

Pressure 1 = P1 = 783 mmHg           Pressure 2 = 735 mmHg

Process

1.- Convert temperature to °K

T1 = 19 + 273 = 292°K

T2 = 37 + 273 = 310°K

2.- Use the combined gas law to solve this problem

                 P1V1/T1  = P2V2/T2

-Solve for V2

                 V2 = P1V1T2 / T1P2

-Substitution

                 V2 = (783 x 4.40 x 310) / (292 x 735)

-Simplification

                V2 = 1068012 / 214620

-Result

                V2 = 4.97 l

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