The Latent Heat of Vaporization for water is L-540 cal/g 2.26x10 J/kg. If 300 g of water went from room temperature, 220C, to 50°C in the calorimeter, how much steam (expressed in grams) would be produced? Briefly describe the physical phenomena that are involved in this process.
The heat of vaporization of water is 540 cal/g, and the heat of fusion is 80 cal/g. The heat capacity of liquid water is 1 cal g−1 °C−1, and the heat capacity of ice is 0.5 cal g−1 °C−1. 18 g of ice at -6°C is heated until it becomes liquid water at 40°C. How much heat was required for this to occur?
Suppose data for latent heat of vaporization is as follows: initial water temperature = 19.50 degrees Celsius, final water temperature = 41.20 degrees Celsius, initial water mass = 65.10 g, final water mass = 67.30 g. Present an algebraic expression for the latent heat of vaporization (Lv).
The specific heat of silver is 0.057 calories/gram°C. If 10.0 grams of silver were heated and the temperature of the sample changed by 20.0°C, how many calories of heat energy were absorbed by the sample? (A)3,508 calories (B)0.029 calories (C)11.4 calories (D)0.114 calories
How many calories are needed to convert 125 grams of water at 75.0 C to steam at 100.0 C? [Specific heats: ice = 0.495, water = 1.00 steam = 0.478 cal/g C] [water's heat of fusion = 80.0 cal/gram, water's heat of vaporization - 540.0 cal/gram] 3125 cal 3330 cal 6875 cal 13,125 cal 70,625 cal
The latent heat of vaporization of H2O at body temperature (37.0 °C) is 2.37E+6 J/kg. To cool the body of a 77.9 kg jogger [average specific heat capacity = 3450 J/(kg·°C)] by 1.70 °C, how many kilograms of water in the form of sweat have to be evaporated?
The heat of vaporization is 540 cal/g. How many kilocalories are needed to change 5.2 g of liquid water to steam at 100°C. Treat as exact
PRE-LAB FORM LATENT HEAT AND SPECIFIC HEAT 1. What is your explanation of heat? 2. What is a calorimeter? 3. Define the specific heat. 4. Define the latent heat of fusion and the latent heat of vaporization. 5. In an experiment 70 gram of ice at 0 °C is dropped into 300 gram of water at 50 °C. Assuming that the calorimeter prevents heat flow to the surroundings, what is the final temperature of thermal equilibrium? (Ignore the calorimeter.)
What is a liquid's heat of vaporization? It is the amount of heat needed to vaporize one liter of the liquid at its boiling point. It is the amount of heat needed to melt one gram of the liquid at its freezing point. It is the amount of heat needed to vaporize one gram of the liquid at its boiling point. It is the amount of heat needed to vaporize one kg of the liquid at its boiling point.
The latent heat of vaporization of H2O at body temperature (37.0°C) is 2.37E+6 J/kg. To cool the body of a 74.6 kg jogger [average specific heat capacity = 3480 J/(kg*°C)] by 1.20°C, how many kilograms of water in the form of sweat have to be evaporated?