Heating curve for water

0:00- [Instructor] Let's look at the heating curve for water. A heating curve has temperature on the y-axis. In this case, we have it in degrees Celsius. And heat added on the x-axis, let's say it's in kilojoules. Let's say we have 18.0 grams of ice and our goal is to calculate the total heat necessary to convert that 18 grams of ice at -25 degrees Celsius to steam at 125 degrees Celsius.

0:28So we're starting with ice at -25 degrees Celsius and first we need to heat up the ice to zero degrees Celsius, which we know is the melting point. So on our heating curve, we're going from point A to point B. To calculate the heat necessary, we need to use the equation Q is equal to mc delta T, where q is the heat added, m is the mass of the ice.

0:53c is the specific heat of ice and delta T is the change in temperature, which is the final temperature minus the initial temperature. So we're trying to calculate q. We know the mass of our ice is 18.0 grams. The specific heat of ice is 2.03 joules per gram degrees Celsius.

1:18And for the change in temperature, it's final minus initial. So the final temperature would be zero degrees Celsius, initial is -25. So zero minus -25 gives us +25 degrees Celsius. So grams will cancel out, degrees Celsius cancels out. And this gives us q is equal to 9.1 times 10 to the second joules to two significant figures or we could also write 0.91 kilojoules.

1:55Now that the ice is at zero degrees Celsius, we know what's going to melt. So we're gonna go from point B on the heating curve to point C. And to calculate how much heat is necessary to melt the ice, we need to know the heat of fusion of ice, which is equal to 6.01 kilojoules per mole.

2:18So we need to figure out how many moles of ice we have. After starting with 18.0 grams, we divide by the molar mass of H2O which is 18.0 grams per mole. And the grams will cancel and give us one mole. So we have 1.00 moles of ice and we multiply that by 6.01 kilojoules per mole and the moles cancel out and give us 6.01 kilojoules.

2:50Now that all the ice is melted, we have liquid water. And so on our heating curve, we're gonna heat that liquid water from zero degrees Celsius to 100 Celsius which is the boiling point of water. So we're going from point C to point D on the heating curve. To calculate the heat added, we use the Q is equal to mc delta T equation again.

3:12So we're solving for Q. The mass is still 18.0 grams but the specific heat now, since we have liquid water, we need to use the specific heat of liquid water, which is 4.18 joules per gram degrees Celsius. And for the change in temperature, the final temperature is 100.

3:34So 100 minus zero gives us +100 degrees Celsius. So grams cancel out, degrees Celsius cancels out and we find that Q is equal to 7.52 times 10 to the third joules, let me just correct three there, 7.52 times 10 to the third joules, which is equal to 7.52 kilojoules.

4:07Once we reached a point D in the heating curve, we're at the boiling point of water. So the heat that we add now is gonna go into turning the liquid water into gaseous water. So going from point D to point E, we're doing a phase change. We need to know the heat of vaporization of water, and that's equal to 40.7 kilojoules per mole.

4:31And we already know we have one mole of H2O. So one mole times 40.7 moles, the moles cancel and it takes 40.7 kilojoules of energy to convert the liquid water in to gaseous water or steam. Next we're gonna heat the gaseous water from 100 degrees Celsius to 125 degrees Celsius.

4:55So we're going from point E to point F on the heating curve. And to figure out how much heat we need to add, we use the Q is equal to mc delta T equation one more time. So we're solving for Q and we still have 18.0 grams. This time we need to use these specific heat of steam, which is 1.84 joules per gram degree Celsius.

5:20The change in temperature would be 125 minus 100 or +25 degrees Celsius. So grams cancel, units cancel out and we get Q is equal to 8.3 times 10 to the second joules to two significant figures, which is equal to 0.83 kilojoules. Finally, we need to add everything up.

5:50So going from point A to point B in the heating curve. So think about just the X axis this time, all right? So going from point A to point B, we calculated that to be equal to 0.91 kilojoules. And then from point B to point C, we calculated that to be 6.01 kilojoules.

6:13From C to D, so this distance here was 7.52. From D to E, this was the big one here. This was equal to 40.7 kilojoules. And finally from E to F we calculated this was equal to 0.83 kilojoules. And when you add everything up this is equal to 56.0 kilojoules. So that's how much energy it takes to convert 18.0 grams of ice at -25 degrees Celsius to gaseous water at 125 degrees Celsius.

6:58Next, let's think about the slopes of the different lines on our heating curve. So let's look at the line going from B to C and also the line going from point D to point E. Both of these lines represent phase changes, going from point B to point C was going from a solid to a liquid and going from point D to E was going from a liquid to a gas.

7:22And since the slope of both of these lines is zero, that means as you add heat on the x-axis, the temperature doesn't change. So during a phase change, all the energy goes into disrupting the intermolecular forces that are present and they don't go into increasing the temperature.

7:42So there is no increase in temperature during a phase change. Think about going from point D to point E, this was converting our liquid water into gaseous water. So as the heat is being added, all that energy goes into breaking the intermolecular forces between water molecules and pulling apart those liquid water molecules and turning them into gaseous water molecules.

8:06So it's only after all of the liquid water molecules are converted into gaseous water molecules, that's when we see the temperature increase again. So talking about from point E to point F, everything is now in the gaseous state and then we see the increase in temperature.

8:22Finally, let's compare the slope of the line from A to B to the slope of the line from C to D. If we look at it, the slope of the line from A to B is a little bit steeper than the slope of the line from C to D. The reason for the different slopes has to do with the different specific heats.

8:41From A to B, we used the specific heat for ice which is 2.03 joules per gram degrees Celsius. From C to D in our calculation, we used the specific heat for water which is 4.1 joules per gram degrees Celsius. The higher the value for the specific heat, the more energy it takes to raise the temperature of a substance by a certain amount.

9:06So if we think about comparing these two, let's say we try to raise the temperature of ice by 25 degrees Celsius. So lets think about this distance here on the y-axis. We would have to put in only a small amount of energy to get ice to increase its temperature by 25 degrees Celsius.

9:23We think about that same temperature change on liquid water. So if we tried to increase the temperature of liquid water by that same amount, 25 degrees, we would have to put in more energy. So on the x-axis, we have to put in more energy to accomplish the same change in temperature.

9:40And that's because liquid water has a higher specific heat. Since it might be a little bit hard to see on that diagram, let's think about putting some heat into a substance here. So I'm gonna draw a horizontal line, and then we're trying to accomplish a certain temperature change.

9:55So I'll draw a vertical line. Those two give me a line with a slope. So let's say we're trying to accomplish the same change in temperature. So I'll draw this Y distance the same as before but we have a higher specific heat. So it takes more energy. Therefore this X distance is going to increase.

10:17And when we increase the X distance, we see that the slope decreases. So the greater the value for the specific heat, the lower the slope on the heating curve.