E.
Molar mass of butane, C4H10 = 58 g / mol
Heat of vapourization of butane = 21.3 kJ / mol
So,
Heat of vaporization of 58 g. of butane = 21.3 kJ
Then,
Heat of vaporization of 245 g. of butane = 245 x 21.3 / 58 = 90.0 kJ
F.
Moles of butane, n = Mass / Molar mass = 245 / 58 = 4.22 mol
Pressure, P = 760 torr = 1 atm
Temperature, T = 37 + 273 = 310 K
R = 0.0821 L.atm / K.mol
Volume, V = ?
Ideal gas equation,
P V = n R T
1 x V = 4.22 x 0.0821 x 310
V = 107. L
How much heat must be added to vaporize 245 g of butane if its heat of...
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