Hello, I have a question about the task:
How many liters of water would be needed to absorb this amount of heat? (Heat capacity: 4.2 kJ/kg K)
I had 31818 kj out in the previous heat
given are still T=70 degrees, T=25 degrees
I thought that I could perhaps get the result with the formula Q=m*Cp*deltaT if I simply rearrange the formula for m… but how do I then get the volume?
(2 votes)
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One of the few material constants that one should have in the head: 1 kg of water has quite exactly the volume 1 l=1 dm3 at customary temperatures.
Mass by density equal volume
density 997.04 kg/m3.at 25°C
0,99704 kg per liter
Thank you
Do you really think it’s 5 digits for r/important, while the heat capacity has only 2 digits?
As long as it is not otherwise required, the density of water is 1.0 kg/L
No, I always reckon with 1.0.
Just wanted to clarify that there are differences for some acutely dizzying teachers.
You’re right.