Just before I delve into my question I'm just gonna say, I think my misunderstanding has to do with 1) the definition of a calorie and 2) how energy and temperature work together.
So, my textbook says that a calorie is how much energy one would need to raise the temperature of 1g of water 1°C (also 4.184 joules), is this not true?
BUT, it is also tells me a page later, in the context of heat of vaporization, that it takes 580 calories to evaporate 1g of water that is 25°C. From the definition of a calorie, wouldn't it be 75 calories to evaporate it? Also, the reason why they say this is to show water's high heat of vaporization due to hydrogen bonding, does it have to do with that?
Just before I delve into my question I'm just gonna say, I think my misunderstanding has to do with 1) the definition of a calorie and 2) how energy and temperature work together. So, my textbook says that a calorie is how much energy one would need to raise the temperature of 1g of water 1°C (also 4.184 joules), is this not true? BUT, it is also tells me a page later, in the context of heat of vaporization, that it takes 580 calories to evaporate 1g of water that is 25°C. From the definition of a calorie, wouldn't it be 75 calories to evaporate it? Also, the reason why they say this is to show water's high heat of vaporization due to hydrogen bonding, does it have to do with that?