A sample of sulfur dioxide (SO2) is initially at a temperature of 155°C, a volume of 25 L, and a pressure of 950 mm Hg. If the
volume changes to 30 L and the temperature increases to 200°C,
what is the new pressure? Show your work.
Show your work. Don't forget to convert °C to Kelvin.

874.89 mmHg

Explanation:

Using the combined gas law equation as follows:

P1V1/T1 = P2V2/T2

Where;

P1 = initial pressure (mmHg)

P2 = final pressure (mmHg)

V1 = initial volume (L)

V2 = final volume (L)

T1 = initial temperature (K)

T2 = final temperature (K)

Based on the information provided in this question;

P1 = 950 mm Hg

P2 = ?

V1 = 25 L

V2 = 30 L

T1 = 155°C = 155 + 273 = 428K

T2 = 200°C = 200 + 273 = 473K

Using P1V1/T1 = P2V2/T2

950 × 25/428 = P2 × 30/473

23750/428 = 30P2/473

55.49 = 0.063P2

P2 = 55.49 ÷ 0.063

P2 = 874.89 mmHg

1.43 x 10^-11 j the guy commented the awnser just making sure u see it .