Exactly 10.0 mL of water at 25.0^∘ C is added to a hot iron skillet. All of the water is convert

Exactly 10.0 mL of water at 25.0^∘ C is added to a hot iron...

Exactly $10.0 \mathrm{mL}$ of water at $25.0^{\circ} \mathrm{C}$ is added to a hot iron skillet. All of the water is converted into steam at $100.0^{\circ} \mathrm{C}$ The mass of the pan is $1.20 \mathrm{kg} .$ What is the change in temperature of the skillet?

Key Concepts

Specific Heat Capacity

Specific heat capacity is a material property that defines the amount of energy required to raise the temperature of a unit mass of a substance by one degree Celsius. It plays a key role in determining how much heat is absorbed or released when a substance’s temperature changes.

Latent Heat

Latent heat refers to the energy absorbed or released during a phase change of a substance at a constant temperature and pressure. In this context, the latent heat of vaporization for water quantifies the energy required to convert liquid water into steam without changing temperature.

Conservation of Energy in Calorimetry

Conservation of energy in calorimetry involves the principle that the energy lost by a hot object (such as the skillet) must be equal to the energy gained by a cooler substance (like water), including both the energy for raising its temperature and the energy for its phase change. This principle is used to determine how the temperature of one component of a system is affected by the energy exchange with another.

Transcript

00:01 Hello, so here we are going to calculate the change in temperature of a skylight pan when we add a specific amount of water at 25 degrees in the pan.

00:13 So first of all, let's write down all the information we have, so we know that we have 10 mils of 25 degree hot water, and we also know that water when it's liquids, converted to gas, so steam at 100 degrees celsius and we know that the mass of the pan is 1 .2 kilograms.

00:53 So first of all, what we need to do here is calculate the heat required, the heat absorbed by the water when it reaches 100 degrees from 25.

01:04 So basically, when it's, when it reaches 100 degrees from 25.

01:06 So basically, when we add the water in the pan and what's the heat required to take it to 100 % celsius degrees temperature.

01:18 So in order to do that, we're going to use the equation q equal m, c, delta, t.

01:26 So we need to calculate q, which is the heat i'm talking about.

01:30 M is the mass of water.

01:32 C is a specific heat of water of 25 degrees and delta t is a change in temperature.

01:38 So q equals m with the mass of water is 10 grams because the concentration of water is 1 gram per mill times the specific heat, which is 4 .18 times that 75 degrees change from 25 to 100.

02:09 Kilojoules.

02:10 So that's all the heat required to basically get the water temperature that can be converted to steam.

02:18 However, what we need to do now is also calculate the vaporization energy of water.

02:27 And that's 40 .70 kilojoules per mole.

02:37 And we need to calculate the exact kilojoules for.

02:42 The amount of water we have in this problem.

02:45 So what we are going to do is basically times the 40 .7 kilojoules per mole and times that by m, the mass of water, which is 10, over the mr, which is 18.

03:02 And that will give us the amount of moles of water we have in this situation...

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