Question

A chemist mixes 75.0 g of an unknown substance at 96.5°C with 1,150 g of water at 25.0°C. If the final temperature of the system is 37.1°C, what is the specific heat capacity of the substance? Use 4.184 J / g °C for the specific heat capacity of water. I need an explanation to this question not solution...

Answer 1

Asked and answered here:
https://questioncove.com/updates/4fa6f6a0e4b029e9dc366363
Also keep in mind heat lost = heat gained

Answer 2

That's just teh solution, I need explanation for this question...

Answer 3

Ok wait. You need a explaination but to what exactly, The solution to the problem?

Answer 4

To elaborate on my solution from the other post

q = mC(Tf-Ti)

where q is heat, C is specific heat, Tf is final temperature, Ti is final temperature

all the heat that was lost from the unknown substance is gained by the water

heat lost by the substance q = -75.0(C)(37.1-96.5)
heat gained by the water: q = 1150(4.184)(37.1-25)

set them equal to each other and solve for C

Answer 5

Yes I need a scientific explanation rather than mathematical reasoning or solution

Answer 6

"all the heat that was lost from the unknown substance is gained by the water" this is a very good explanation but could you just elaborate and add more explanation to this

Answer 7

Energy is conserved. When the substance is added to water, it loses some amount of heat. That same amount of heat is added to the water.

Since we know: the mass of the water, the specific heat of the water, and the temperature change of the water, we know how much heat the water gained via q = mc delta T

We can then use that heat to solve for the specific heat of the substance

Answer 8

thank you