∙How much heat is required to convert 12.0 g of ice at -10.0^∘ C to steam at 100.0^∘ C ? Express

step 1 In this problem we're going to talk about heat. And there are basically two types of heat we're

∙How much heat is required to convert 12.0 g of ice at...

Key Concepts

Specific Heat Capacity

Specific heat capacity is the amount of energy required to raise the temperature of a unit mass of a substance by one degree Celsius (or one Kelvin). It is a key concept in calorimetry and is essential for calculating the energy needed to heat or cool substances without a phase change.

Latent Heat

Latent heat refers to the heat absorbed or released during a phase change (e.g., melting, freezing, boiling, or condensation) of a substance, occurring without any change in temperature. This concept is fundamental when calculating energy changes during transitions between solid, liquid, and gas states.

Heat of Fusion

The heat of fusion is the latent heat required to change a substance from a solid to a liquid at its melting point. It represents the energy needed to break the bonds in a solid structure, such as converting ice into water.

Heat of Vaporization

The heat of vaporization is the latent heat necessary to convert a liquid into a gas at its boiling point. It indicates the substantial energy input required to overcome the intermolecular forces in a liquid, exemplified by the conversion of water to steam.

Energy Unit Conversion

Energy unit conversion involves transforming energy values from one unit system to another, such as converting joules to calories using the factor 1 calorie ? 4.184 joules. This capability is important for ensuring consistency across different scientific contexts and applications.

Transcript

00:01 In this problem we're going to talk about heat.

00:02 And there are basically two types of heat we're going to be interested in in our problem.

00:08 First, the heat necessary to change the temperature of an object.

00:15 I'm going to call it just q and it's equal to the mass of the object times the specific heat, c of the object, times the change in temperature.

00:27 So if the temperature is raised, the heat necessary, to do so is positive if the temperature is lowered the heat that the object loses is negative.

00:41 Also, there is the latent heat i'm going to call a q -o -l that is necessary to change the face of matter of an object.

00:55 So, for example, if we have solid ice and we want to transform it to liquid water, that process happens.

01:03 At zero kelvin, so there is no heat related to the difference in temperature, but there is a heat, there is a heat, i'm sorry, related to the fact that the water is changing its face.

01:20 So ql, the latent heat, is equal to the latent heat constant l times the mass of the object, and now we can go on to our problem.

01:31 Basically we have a mass of 12 grams of water that is initially at a temperature of minus 10 degrees celsius and we want the final state of the water to be vapor at a temperature of 100 degrees celsius so notice some things first i'm going to write here the specific heat of the water which is 4 .182 joules per kelvin gram.

02:11 And also the latent heat of fusion, that is when the water changes from being ice to being liquid water, it's equal to 334 joules per gram.

02:28 And the latent heat of vaporization, the name tells it all, it's when the water converts from being liquid to being gas.

02:36 This is equal to 2 ,260 joules per gram.

02:45 Okay, so notice that we have the following process.

02:51 We have water at minus 10 degrees celsius.

02:54 Then we have the heat...

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