Calculating Heat Requirements for Phase Changes

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To determine which process requires more heat, the Latent Heat of Fusion for melting ice is 80 cal/gram, while the Latent Heat of Vaporization for turning water into steam is 540 cal/gram. Melting 500 g of ice at 0°C requires 40,000 calories, while converting 500 g of water at 100°C to steam requires 270,000 calories. Therefore, turning water into steam requires significantly more heat than melting ice. Understanding these concepts is crucial for solving similar problems in thermodynamics. Mastering the calculations will aid in grasping the overall material in the online class.
momtonate
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I have no clue how to do this?

Which would require more heat, melting 500 g of 0 C ice or turning 500 g of 100 C water into steam?
 
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momtonate said:
I have no clue how to do this?

Which would require more heat, melting 500 g of 0 C ice or turning 500 g of 100 C water into steam?
You need to know the Latent Heat of Fusion (80 cal/gram) for {Ice → Liquid Water} transition and the Latent Heat of Vaporization (540 cal/gram) for {Liquid Water → Steam} transition. Can you answer the question now??


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I still am not sure what to do...I am taking an online class and we basically have to learn the material ourselves. So if I can get help with just one then I can figure the rest out.
 
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