"Volcanos can exist on glaciers where the temperatures can reach -70.0 degrees C at night. How many kcal and kJ of heat are absorbed by a 2.4 kg chunk of ice on the surface (-70.0 C) that is converted to steam at 300 C after the ice falls into a chamber inside the volcano. (Hint: The ice must be warmed, melted, warmed again, vaporized to steam, and finally warmed again) (the heat capacity of ice = 0.51 cal/g*C and the heat capacity of steam is 0.48 cal/g*C)."

Would I use the heat equation for this problem?
heat = 2.4g * 230 C * 0.51cal/g*C = 280 cal

Am I going in the right direction?

Question

"Volcanos can exist on glaciers where the temperatures can reach -70.0 degrees C at night. How many kcal and kJ of heat are absorbed by a 2.4 kg chunk of ice on the surface (-70.0 C) that is converted to steam at 300 C after the ice falls into a chamber inside the volcano. (Hint: The ice must be warmed, melted, warmed again, vaporized to steam, and finally warmed again) (the heat capacity of ice = 0.51 cal/g*C and the heat capacity of steam is 0.48 cal/g*C)." 

Would I use the heat equation for this problem? 
heat = 2.4g * 230 C * 0.51cal/g*C = 280 cal 

Am I going in the right direction?

wolfe8 · Answer

Welcome to OpenStudy. Oh no you don't just multiply it with the temperature(you calculated the difference wrong too). You know Q=cmdT where dT is the change in temperature and c is the specific heat capacity. And note that the temperature change goes from -70 to, then from 0 to 100, then 100 to 300.

wolfe8 · Answer

And you should use 3 c's here in 3 different calculation before adding them up, because you are going through 3 different phases of water.

anonymous · Answer

Thank you!

wolfe8 · Answer

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