Problem: If 42.0 kJ of heat is added to a 32.0-g sample of liquid methane under 1 atm of pressure at a temperature of -170oC, what is the final state of the methane once the system equilibrates? Assume no heat is lost to the surroundings. The normal boiling point of methane is -161.5 oC. The specific heats of liquid and gaseous methane are 3.48 and 2.22 J / g, respectively.

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If 42.0 kJ of heat is added to a 32.0-g sample of liquid methane under 1 atm of pressure at a temperature of -170oC, what is the final state of the methane once the system equilibrates? Assume no heat is lost to the surroundings. The normal boiling point of methane is -161.5 oC. The specific heats of liquid and gaseous methane are 3.48 and 2.22 J / g, respectively.

There are 32.0 grams of liquid methane (CH4) inside a chamber in a cylinder with a piston. Delta Hvaporization is 8.20 kilojoules per mole and temperature is negative 170 degrees Celsius. The downward pressure on the piston is equal to 1.00 atmospheres, while 42.0 kilojoules of heat are added to the chamber in the cylinder.


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