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Heat of vaporization is the heat required to vaporize unit mass of a substance at it's boiling point. The heat of vaporization or condensation of water is 2257 J/g.
It means that 1 g of water involves 2257 J energy during condensation or vaporization at its boiling point (100 C)
Given mass of water vapor that is condensing = 11.2 g
Calculating the heat released when 11.2 g of water vapor condenses in to liquid water at 100:
Rounding the final answer 25,278 J to three significant figures we get, 25,300 J
Therefore the correct answer is E. 25,300 J
Answer : The new pressure if the sample placed in a 2.00-L container is, 0.494 atm.
Explanation :
Boyle's Law : It is defined as the pressure of the gas is inversely proportional to the volume of the gas at constant temperature and number of moles.
or,
where,
= initial pressure = 0.988 atm
= final pressure = ?
= initial volume = 1.00 L
= final volume = 2.00 L
Now put all the given values in the above equation, we get:
Thus, the new pressure if the sample placed in a 2.00-L container is, 0.494 atm.