The discussion centers on a thermodynamics problem involving a 2.00 kg solid cube of nitrogen at -220.0°C mixed with a 1.00 kg mixture of ice and water at 0.00°C, resulting in a final temperature of -100.0°C. The key equations used are e=mct for calculating heat transfer and e=mLv/f for latent heat. A critical calculation involves determining that 476,400 Joules of energy is required to raise the nitrogen to -100°C. Additionally, the properties of nitrogen are clarified, noting its phase changes at specific temperatures.
PREREQUISITESStudents studying thermodynamics, physics educators, and anyone involved in heat transfer calculations in physical chemistry or engineering contexts.
heat gained = heat lostZoey Brown said:Homework Statement
A solid, 2.00 kg cube of nitrogen at -220.0oC is added to a 1.00 kg mixture of ice and
water at 0.00 oC. If the final temperature of the mixture is -100.0 oC, how much ice was
there in the original mixture?
Homework Equations
e=mct
e=mLv/f
The Attempt at a Solution
Don't know where to start
Did you remember that N2 is liquid below -196C and gas above that temperature?Fizzix_G said:Hi Zoey,
First you have to start off by calculating how much energy it takes to make nitrogen go to -100 degrees Celsius. Try doing this and the number you should get is 476 400 Joules.