Homework Answers
Ideal gas equation,
PV = nRT
P (250.0mL x 1 L / 1000 mL) = (0.3400 g C6H6 x 1 mol C6H6 /78.11 g C6H6)0.0821 L.atm/(mol.K) [333 K]
P = 0.476 atm
Given that the vapor pressure of benzene at this temperature is 400.0 torr
The given pressure = 0.476 atm = 0.476 atm x 760 torr / 1 atm = 361.76 torr
Pressure (361.76 torr) of benzene in the container is less than it's vapor pressure (400.0 torr). Hence all of the benzene will be in liquid state (doesnot vaprize).
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Combustion of 4.93 g of liquid benzene (C_6H_6) causes a temperature rise of 20.9 degree C in a constant pressure calorimeter that has a heat capacity following reaction? -41.8 kJ/mol-rxn 41.8 kJ/mol-rxn -3.27 times 10^3 kJ/mol-rxn 206 kJ/mol-rxn 206 kJ/mol-rxn What is the correct formula for gallium (III)peroxide? Ga(O_2)_2 Ga_2(O_2)_3 Ga_3(O_2)_2 Ga_2O_2 GaO_2
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At 25°C, the vapor pressure of benzene is 13.1 kPa. A sample of 0.20 g of benzene is injected into an evacuated flask with a volume of 250 ml. What mass of liquid benzene remains after equilibrium is established. You may ignore the volume taken up by the liquid benzene in the flask. Numeric Answer.
Diethyl ether, C4H100 was a widely used anesthetic in the early days of surgery. It has a vapor pressure of 537 torr at 25 °C. A 10.00 mL sample (D = 0.708 g/mL) is placed in a sealed 0.205 L flask. What is the maximum volume in liters the flask can have if equilibrium is to be maintained between liquid and vapor?
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