Question

(The question is in the photo Sorry) A sample of gas occupies 7 mL at STP. At what pressure would this sample occupy 500 mL if the temperature is changed to 525°C?Answer in units of torr.✨Please leave all the numbers after the decimal & do not round

Answer 1

Given:

V1 = 7 mL

V2 = 500 mL

T2 = 525 degrees celsius = 525 + 273 = 798

We know that at STP:

T1 = 0 degrees celsius = 273 K

P1 = 1 atm = 760 torr

We want the final pressure in torr. We have to first convert 1 atm to torr.

1 atm = 760 torr

We also need to convert T from degrees celsius to K

We will use the following equation:

$\frac{P_1V_1}{T_1}\text{ = }\frac{P_2V_2}{T_2}$

P2 = (760 torr x 7 mL x 798 K)/(500 mL x 273 K)

P2 = 31.10153846 torr