# Newcomer Asks: What is the Final Temperature?

• Msnyder
In summary: ERICAN MATH CORE: Heat is lost when an object changes temperature. The amount of heat lost is equal to the amount of heat gained.

#### Msnyder

First time here so be easy please!

Problem: What would final temp. be when 100g of 25C water is mixed with 75g of 40c water?

Do I use deltaT=deltaQ/cm?

If there is a more basic forum, please let me know, I do not want to offend anyone.

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Yep, that's the equation to use.

any help would be appreciated, I am getting confused with the problem

somehow I am getting 15C/175,000?

By the way, if there is a more basic forum, let me know...I do not want to offend anyone!

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what did you do to get that answer?

the heat released by the hotter portion is the heat gained by the cooler portion. that's where I'd start solving the problem from.

addition: maybe this should be in some of the homework forums? otherwise it's in the right place. if this is in the wrong place don't start a new thread but wait for a moderator to move it to the right place.

I understand that heat lost is = to heat gained,but what about the added water?

I guess the better question would be, what is the c of water?

**I feel like a 10 yr old boy in this class!

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c is 4.19kJ/kg*K.

Think in terms of conservation of energy. If no energy is lost then the Q of the final state (175 grams of water at some temperature T) must be equal to... You fill the blank.

Quick questions, do I average the temps or do I subtract 40 -25 which is 15C. Are you saying that the water conserves it's energy, so the addition of mass does not matter, it's just 15C?

Don't be confused by the fact that you're mixing water with water. In the end (at thermal equilibrium) both 'parts' share the same temperature. Call it T.
Using this T, what is the amount of heat 1 part of the water gained, what is the amount of heat the other one gained? What should T be such that the total amount of heat gained is zero?

wow...I guess one gained 15 degrees and the other gained nothing, so together they gain 15, because the transfer of heat is from the hotter to the cooler?

So, from the original problem, the water ends up at 40 degrees?

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Thanks for your help everyone, but I am not getting anywhere. This is just extra hard for me at this point. I will try my text again and see if I can come up with something. Thanks again,
Mike

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Msnyder said:
Thanks for your help everyone, but I am not getting anywhere. This is just extra hard for me at this point. I will try my text again and see if I can come up with something. Thanks again,
Mike
Think of the problem this way:

Begin with 175 g of water at 25 deg. C and add heat that is sufficient to warm 75g of water to 40 degrees (ie. 75 g x 15 deg = 1125 Cal). What is the temperature raised by? (ie. 1125 Cal into 175 g = ? deg).

AM

## 1. What factors affect the final temperature in a system?

The final temperature in a system is affected by several factors, including the initial temperatures of the components, the amount of energy added or removed from the system, the specific heat capacities of the components, and the rate of heat transfer.

## 2. Can the final temperature ever be lower than the initial temperature in a system?

No, the final temperature in a system can never be lower than the initial temperature. This is because of the law of conservation of energy, which states that energy can neither be created nor destroyed, only transferred. Therefore, the total energy in a closed system will always remain constant, meaning the final temperature will never be lower than the initial temperature.

## 3. How does the type of container affect the final temperature in a system?

The type of container can affect the final temperature in a system by influencing the rate of heat transfer. For example, a container made of a good conductor, such as metal, will allow for faster heat transfer compared to a container made of a poor conductor, such as plastic. This can result in different final temperatures in the system.

## 4. Is the final temperature always the average of the initial temperatures in a system?

No, the final temperature in a system is not always the average of the initial temperatures. This is because the specific heat capacities of the components can vary, meaning some components will require more energy to reach the same temperature as others. Additionally, the rate of heat transfer can also affect the final temperature, resulting in a non-average value.

## 5. How can the final temperature be calculated in a system?

The final temperature in a system can be calculated using the law of conservation of energy, which states that the total energy in a closed system remains constant. This means that the sum of the energies of all components before and after the energy transfer must be equal. By setting the initial and final energies equal and solving for the final temperature, the final temperature in the system can be determined.

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