If 115 grams of water at 25 degrees C absorbs 285 kJ of heatfrom a mountain clim

Question

If 115 grams of water at 25 degrees C absorbs 285 kJ of heatfrom a mountain climber's stove at an elevation where the boilingpoint of water is 93 degrees C, is this amount of energy sufficientto heat the water to its boiling point?   Yes orno? How many kJ are required to boil the water? If 115 grams of water at 25 degrees C absorbs 285 kJ of heatfrom a mountain climber's stove at an elevation where the boilingpoint of water is 93 degrees C, is this amount of energy sufficientto heat the water to its boiling point?   Yes orno? How many kJ are required to boil the water?

Explanation / Answer

Amount of heat required to raise the temperature of water from25 oC to 93 oC is Q = mC dt    = 115 g * 4.184 J / g oC * ( 93-25 )oC    = 32718.88 J    = 32.71888 kJ Yes , The given amount of energy sufficient to heat thewater to its boiling point. No.of kJ of heat required to boil the water = 32.71888kJ

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