A gas sample has an initial volume of 55.2 mL, an initial temperature of 35.0 °C, and an initial pressure of 735 mm Hg. The volume is decreased to 48.8 mL and the temperature is increased to 72.5 °C. What is the final pressure?

The answer to your question is   P2 = 932.6 mmHg

Explanation:

Data

Volume 1 = V1 = 55.2 ml

Temperature 1 = T1 = 35°C

Pressure 1 = P1 = 735 mmHg

Volume 2 = V2 = 48.8 ml

Temperature 2 = T2 = 72.5°C

Pressure 2 = P2 = ?

Process

1.- Convert temperature to °K

Temperature 1 = 35 + 273 = 308 °K

Temperature 2 = 72.5 + 273 = 345.5°K

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

               P1V1/T1 = P2V2/T2

-Solve for P2

               P2 = P1V1T2 / T1V2

-Substitution

               P2 = (735 x 55.2 x 345.5) / (308 x 48.8)

-Simplification

               P2 = 14017626 / 15030.4

-Result

               P2 = 932.6 mmHg

i just calculated it all out, and not including weekends, and all the different days off. as of this school year (2018-2019) students are spending 2198 hours in school this year