29.2 kJ of heat is required to convert an 50.0 g sample of
acetaldehyde from the liquid to gas phase. The molecular
weight of acetaldehyde is 44.05 g/mol. What is the heat of
vaporization of acetaldehyde in kJ/mol?
kJ/mol

The heat of  vaporization of acetaldehyde is 25.72 kJ/mol.

Explanation:

Mass of acetaldehyde = 50.0 g

Molar mass of acetaldehyde = 44.05 g/mol

Moles of acetaldehyde =

Amount of energy required to vaporize 50.0 grams of acetaldehyde = Q

Q = 29.2 kJ

The heat of  vaporization of acetaldehyde :

the tides are influenced by both the moon and the sun, it's easy to see that when the sun lines up with the moon and the earth, as during a new moon or full moon, the tidal effect is increased. these are known as spring tides, named not for the season, but for the fact that the water "springs" higher than normal. on the other hand, if the sun and the moon are 90 degrees apart in relation to an observer on earth as during the first quarter moon or third quarter moon, then high tides are not as high as they normally would be. this is because despite its greater distance, the sun's mass allows it to exert enough gravitational force on the oceans that it can negate some of the effects of the moon's pull. this phenomenon of lower high tides is called a neap tide. if you need more information on this topic visit moonconnection.com.

i think it is true since you can test the answer and can use observations to complete it.