Quick question. Latent heat problem.

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To calculate the heat required to convert 456 g of ice at -25°C to water at 25°C, the total heat (Q) is the sum of the heat needed to warm the ice, the heat for the phase change, and the heat to warm the water. The specific heat of ice (2090 J/kg K) and water (4186 J/kg K) along with the latent heat of fusion (33.5 x 10^4 J/kg) are essential for these calculations. The formula includes Q = m*c*ΔT for both the ice and water, and Qlatent = m*H_f for the phase change. The discussion confirms the correct approach but notes the need for clearer notation. Accurate calculations require careful attention to units and specific heat values.
new324
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Allright, I may sound stupid on this one.
How much heat (Q) is required to change 456 g of ice at -25(degrees celsius) into water at 25(degrees C). The Specific heat of ice is 2090 J/kg K, the specific heat of water is 4186 J/kg K. The latent heat of fusion of water is 33.5*10^4 J/kg.

Is this just going to be Qwater+Qice+Qlatent? Where Qlatent is m*L?
 
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Q = cm\Delta T

and

Q = mH_f

I think you have the right idea, but your notation is a little awkward.

cookiemonster
 
Thanks cookiemonster. I appreciate the help.
 

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