How Much Heat is Needed to Convert Ice at -10C to Steam at 110C?

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    Thermochemistry
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To convert 20.0g of ice at -10°C to steam at 110°C, several steps are required, each involving specific heat calculations. First, heat must be added to raise the temperature of the ice to 0°C, followed by the heat needed to melt the ice into liquid water. Next, the water must be heated to 100°C, then vaporized into steam, and finally, the steam is heated to 110°C. Each phase change and temperature increase requires specific calculations using the given specific heats and heat values for fusion and vaporization. Understanding these steps is crucial for accurately determining the total heat required for the transformation.
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How much heat (in joules) must be added to change 20.0g of H2O(s) at -10C to steam at 110C? The specific heat of H2O(s) is 2.09 J/gC; of H2O(L) is 4.184 J/gC; and of H2O(g) is 1.84 J/gC. The heat fusion of water is 334.7 J/g and the heat vaporization of water is 2259.4J/g.I feel like we have to find the temp for s ---> l and then l ---> g. But I'm completely lost; I don't understand Thermochemistry.
 
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Split it into separate parts - you have to warm up ice till it can be melted, you have to melt it, you have to warm the the water till boiling point, you have to boil it, you finally have to warm up steam. Then add everything.

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