Problem with calculating final temperature of water

In summary, the final temperature of the water in the polystyrene cup is 50°C when a 60 g ice piece is transferred directly from a freezer at -7°C to the cup containing 200 g of water at 75°C. This can be calculated using the equation Qheat ice + Qmelt ice + Qheat cold water + Qcool hot water = 0, where Qheat ice = (0.060 kg) x (2100 J/(kg.C)) x (0°C - (-7°C)), Qmelt ice = ( 0.060 kg) x (3.3 x 10^5), Qheat cold water = (0.060 kg) x (4200 J /(kg
  • #1
v3ra
21
0
A piece of ice with a mass of 60 g is transferred directly from the freezer at a
temperature of –7°C to a polystyrene cup containing 200 g of water at 75°C. Calculate
the final temperature of the water. Ignore any heat loss to the cup and its surroundings.

Qheat ice + Qmelt ice + Qheat cold water + Qcool hot water
mciceΔtice + mLf + mcwΔt + mhwcwΔthw = 0
(0.060 kg) x (2100 J/(kg.C)) x (0°C - (-7°C)) + ( 0.060 kg) x (3.3 x 10^5) + (0.060 kg) x (4200 J /(kg.C)) x (t2 – 0°C) + (0.2) x (4200 J) x (t2 – 75°C) = 0
882 + 19800 + 252t2 + 840t2 – 63000 = 0
840t2 = 42318
t2 = 50°C

The above problem is from my book, but I am having difficulty with the equation. Where did
the 63000 come from?
 
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  • #2
v3ra said:
A piece of ice with a mass of 60 g is transferred directly from the freezer at a
temperature of –7°C to a polystyrene cup containing 200 g of water at 75°C. Calculate
the final temperature of the water. Ignore any heat loss to the cup and its surroundings.

Qheat ice + Qmelt ice + Qheat cold water + Qcool hot water
mciceΔtice + mLf + mcwΔt + mhwcwΔthw = 0
(0.060 kg) x (2100 J/(kg.C)) x (0°C - (-7°C)) + ( 0.060 kg) x (3.3 x 10^5) + (0.060 kg) x (4200 J /(kg.C)) x (t2 – 0°C) + (0.2) x (4200 J) x (t2 – 75°C) = 0
882 + 19800 + 252t2 + 840t2 – 63000 = 0
840t2 = 42318
t2 = 50°C

The above problem is from my book, but I am having difficulty with the equation. Where did
the 63000 come from?

Hi, V3ra. Multiply the three red numbers.
 
  • #3
Hmm, but how would I have known to do that? I already multiplied the 0.2 and 4200 J to get 840. Where in the equation is it implied that I would use these two numbers again along with the 75°C to get 63000?
 
  • #4
It's called the distributive property.
a*(b+c)=a*b+a*c
You have a*(b+c)=a*b
 
  • #5
Can you please elaborate? How would someone who is approaching the above equation for the first time know to apply such a rule? The first part of the equation contains three numbers that are being multiplied, would all three be represented by "a" in the "a*(b+c)=a*b" or is this rule only applying to one part of the equation?
 
  • #6
v3ra said:
Can you please elaborate? How would someone who is approaching the above equation for the first time know to apply such a rule? The first part of the equation contains three numbers that are being multiplied, would all three be represented by "a" in the "a*(b+c)=a*b" or is this rule only applying to one part of the equation?

v3ra, I'm not sure of your question. You are trying to simplify (0.2) x (4200) x (t2 – 75). You noted earlier that you can multiply the 0.2 and the 4200 to get 840. So now you have 840 x (t2-75).

To reduce this, take a simple example: 3 x (6 - 2). This means you have the quantity (6-2) three times.
So, 3 x (6 - 2) = (6-2) + (6-2) + (6-2). So, you get "6" three times and you also get (-2) three times.

So, 3 x (6-2) = 3x(6) + 3x(-2) = 3x6 - 3x2. Thus 3 x (6-2) = 3x6 - 3x2

Likewise, 840 x (t2-75) means that you have 840 of the quantity (t2-75). That's 840 t2 's and also 840 of the quantity (-75).

So, 840 x (t2-75) = 840 x t2 + 840 x (-75) = 840 x t2 - 840x75 = 840t2 - 63000.
 
Last edited:
  • #7
I understand now. I was, for some reason, completely avoiding the "t2".
 
  • #8
No, you had t2, it was the -75 that you left out. That's the term that became the -63000.
 

FAQ: Problem with calculating final temperature of water

1. What is the "problem" with calculating the final temperature of water?

The main problem with calculating the final temperature of water is that it depends on various factors such as the initial temperature of the water, the amount of water, and the specific heat capacity of the container in which the water is heated or cooled. This makes it difficult to accurately predict the final temperature without considering all of these factors.

2. How can the specific heat capacity of the container affect the final temperature of water?

The specific heat capacity of the container can affect the final temperature of water because it determines how much heat energy the container can absorb or release. If the container has a high specific heat capacity, it will require more heat energy to increase its temperature, resulting in a lower final temperature of the water.

3. Is there a formula for calculating the final temperature of water?

Yes, there is a formula for calculating the final temperature of water. It is known as the heat transfer formula and it takes into account the initial temperature, mass, specific heat capacity, and heat transfer coefficient of the water and its surroundings. However, the accuracy of this formula depends on the assumptions made and the variables considered.

4. Why is it important to accurately calculate the final temperature of water?

Accurately calculating the final temperature of water is important in various scientific experiments and processes. In chemistry, it is crucial for determining the energy changes and reactions that occur during heating or cooling of substances. In engineering, it is necessary for designing and optimizing systems that involve heat transfer, such as refrigerators and heat exchangers.

5. What are some potential sources of error when calculating the final temperature of water?

Some potential sources of error when calculating the final temperature of water include inaccuracies in measuring the initial temperature of the water, neglecting the specific heat capacity of the container, and assuming ideal conditions for heat transfer. Other factors such as heat loss to the surroundings and external influences like air currents can also affect the final temperature. It is important to carefully consider all of these factors to reduce errors and improve the accuracy of the calculation.

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