How many moles of chloroform, CHCl3, are required to fill a 253-mL flask at 100.0 C and 940 torr?

0.0103 mole

Explanation:

Data obtained from the question include:

V (volume) = 253mL

Recall: 1000mL = 1L

Therefore, 253mL = 253/1000 = 0.253L

T (temperature) = 100°C = 100 + 273 = 373K

P (pressure) = 940 torr

Recall: 760torr = 1atm

Therefore, 940torr = 940/760 = 1.24atm

R (gas constant) = 0.082atm. L/Kmol

n (number of mole) = ?

Using the ideal gas equation PV = nRT, the number of mole 'n' can be obtained as follow:

PV = nRT

1.24 x 0.253 = n x 0.082 x 373

Divide both side by 0.082 x 373

n = (1.24 x 0.253) / (0.082 x 373)

n = 0.0103 mole

Therefore, the number of mole of chloroform, CHCl3, required to fill the flask is 0.0103 mole

relationship between four fundamental physical properties of gases: pressure PP, volume VV, number of moles nn, and the absolute temperature TT. The ideal gas constant is denoted by RR and its exact value depends on the units chosen for the other parameters. Note that the temperature is always in Kelvins (i. e., we use the absolute temperature). The relation is:

PV=nRT