A 51-g ice cube at 0°C is heated until 43.0 g has become water at 100°C and 8.0 g has become steam at 100°C. How much energy was added to accomplish the transformation? ?kJ
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A 51-g ice cube at 0°C is heated until 43.0 g has become water at 100°C and 8.0 g has become steam at 100°C. How much energy was added to accomplish the transformation?
?kJ
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- Q.13 What happens if you add heat to water that is at the temperature of 100°C? Does the temperature change? Explain.A chocolate bar has 225Cal. Charlie is locked in a deserted chocolate factory and needs to heat 2.00L of water for his dinner. He plans on burning chocolate bars to accomplish this. a) How many kJ of energy are needed to heat the water from 25.0C to 100.0C? __ kJ b) What fraction of a chocolate bar would be needed to heat the water? __% Answer all parts A and B.On a trip, you notice that a 3.15-kg bag of ice lasts an average of one day in your cooler. What is the average power in watts entering the ice if it starts at O°C and completely melts to 0°C water in exactly one day? P = W
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- How much energy is required to change a 30-g ice cube from ice at −25°C to steam at 115°C? ?MJThe initial temperature of 150 g of ice is -20°C. The spe-cific heat capacity of ice is 0.5 cal/g.C° and water's is1 cal/g•C°. The latent heat of fusion of water is 80 cal/g.a.How much heat is required to raisethe ice to 0°C andcompletely melt the ice?b. How much additional heat is required to heat the water(obtained by melting the ice) to 25°C?C.What is the total heat that must be added to convert the80 g of ice at-20°C to water at +25°C?d. Can we find this total heat simply by computing howmuch heat is required to melt the ice and adding theamount of heat required to raise the temperature of 80 gof water by 45°C? ExplainYou are given 3.74 x 10 g of coffee (same specific heat as water) at 83.6°C. In order to cool this to 60.2°C, how much ice (at 0.0°C) must be added? Neglect heat content of the cup and heat exchanges with the surroundings. mice