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

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