Question

can someone please explain how to solve this problem it's slightyly confusing. So far I understand how to set it up but the calculations towards the answer is where im lost

thank you

In a typical gas experiment, a student measured the volume and pressure of a gas generated as 37.45 mL and 21.78 torr, respectively. If the temperature for the day was 31.9 °C, what is the volume of this gas at STP? P, 21.78 torr V, 37.45 mL At STP P 1 atm (760 torr) = P2 0 °C (273.15 K) T T2 T, 31.9 °C (21.78 torr 3745 ml) (760 torr) 31.9 C+27315= 3051 K 27315K 3051 K (760 torr) I 2.673 lorr XmL) 273.15 K 730.1 torr mL = 760 torr xI I, =0.9607 mL 760 torr is an exact number and does not count when figuring out significant figures

Answer 1

Solution:

This question is solved by ideal gas equation. At STP,

Pressure = 760 torr (P2)

Temperature = 273.15 K (T2)

Volume (V2) = ?

Given, that

P1 = 21.78 torr

V1 = 37.45 mL

T1 = 273.15 + 31.9 = 305.05 K

According to ideal gas equation:

P1 V1 / T1 = P2 V2 / T2

Therefore,

V2 = ( P1 V1 T2 )/(P2 T1)

V2 = (21.78 torr x 37.45 mL x 273.15 K) / (760 torr x 305.05 K)

V2 = 0.9610 mL