a) When 0.250 moles of a gas is placed in a container at 25 °C, it exerts a pres

Question

a) When 0.250 moles of a gas is placed in a container at 25 °C, it exerts a pressure of 700 mmHg. What is the volume of the container? (R = 0.0821 L.atm/mol.K)

b) An 18 liter container holds 16.00 grams of a gas at 45 °C. What is the pressure in the container? (molar mass of the gas = 32) (R = 0.0821 L.atm/mol.K)

c) How many moles of hydrogen gas must be placed in a 3.00 liter container in order to exert a pressure of 2.00 atmospheres at 298 Kalvin? (R = 0.0821 L.atm/mol.K)

d) At what temperature (in Kelvin) would 4.0 moles of hydrogen gas in a 100 liter container exert a pressure of 1.00 atmospheres? (R = 0.0821 L.atm/mol.K)

Explanation / Answer

A) V =n*R*T/P =0.25*8.314*298/(700/760*1) =6.64L

(1atm=760 mmHg)

B)P =n*R*T/V =(16/32)*0.0821*318/(18) =0.7252atm

C)n =P*V/(R*T) =2*3/(0.0821*298) =.245 moles

D)T =1*100/(4*0.0821) =304.5 K

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