Mixing Two Liquids: What is the Equilibrium Temp?

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Discussion Overview

The discussion revolves around determining the equilibrium temperature when mixing two liquids of equal mass, one at 50 degrees Celsius and the other at 20 degrees Celsius, with the colder liquid having a higher specific heat. The focus is on the implications of specific heat and mass on the final temperature of the mixture.

Discussion Character

  • Homework-related
  • Debate/contested
  • Mathematical reasoning

Main Points Raised

  • One participant suggests that the equilibrium temperature will be less than 35 degrees Celsius, reasoning that the cooler liquid requires more energy to increase its temperature compared to the energy lost by the hotter liquid.
  • Another participant agrees with the idea that the final temperature must be on the cold side, reinforcing the previous claim.
  • There is a concern raised about the role of volume in the calculations, with one participant questioning whether the ungiven volumes affect the outcome.
  • Clarifications are made regarding the equal masses of the two liquids, with participants acknowledging this point in response to earlier confusion.
  • One participant corrects themselves after realizing their misunderstanding about the relationship between mass and specific heat in this context.

Areas of Agreement / Disagreement

Participants generally agree that the equilibrium temperature will be less than 35 degrees Celsius, but there is some uncertainty regarding the role of volume and specific heat in the calculations. The discussion remains somewhat unresolved due to differing interpretations of the implications of specific heat and mass.

Contextual Notes

There are limitations regarding assumptions about the specific heat capacities and the potential impact of volume on the final temperature, which are not fully explored in the discussion.

metalmagik
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Homework Statement


Two liquids of equal mass, one at 50 degrees Celsius, and one at 20 degrees Celsius, have different specific heats. Suppose the colder liquid has the higher specific heat. If the two liquids are mixed together in an insulating container, the equilibrium temperature of the mixture will be:
(a) 35 degrees C
(b) greater than 35 degrees C
(c) less than 35 degrees C
(d) not enough information


Homework Equations


Q = mc(delta T) ?


The Attempt at a Solution


Now I know there's nothing to really calculate here, so after thinking about this question for about 10 minutes...I thought the answer was (c) less than 35 degrees Celsius. However, after talking to one of my classmates, he brought up the fact that Volume is not given. Then, I told him that volume should really have no bearing on specific heat capacities, since specific heat is defined as the amount of heat needed to change 1g of the substance 1 degree Celsius either higher or lower. So, right now I'm between (c) and (d). Does anyone have the right answer? I even tried googling this after spending all this time deliberating with myself, and with my classmate. Any help is greatly appreciated.
 
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I would say 'C', you know that the cooler liquid must 'win'. It needs more energy to heat by 1deg than the hotter liquid gives by cooling 1deg and so the final temperaturemust be on the cold side.
 
That's what I thought, I just wasn't sure if the ungiven volumes played a role. Thanks mgb_phys!
 
mgb_phys said:
I would say 'C', you know that the cooler liquid must 'win'. It needs more energy to heat by 1deg than the hotter liquid gives by cooling 1deg and so the final temperaturemust be on the cold side.

No - it doesn't take more energy to heat a gram of the cooler liquid by 1 deg. than a kilo of the hotter one gives by cooling 1 deg. !
 
The question says that there are equal masses of the two liquids.
 
mgb_phys said:
The question says that there are equal masses of the two liquids.

Sorry :blushing:I got confused in hurry with another comment. Then mgb is right.
 

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