Calculate the amount of energy given off when 13g of water at 51° C freezes to ice at 0°C. Did a phase change occur? If so, which one? Is this endothermic or exothermic?

Determine the heat in kJ to heat 7.18 moles of ice from -29.286 degrees celcius to -2.357 degrees celcius. the specific heat of ice is 2.03 J/g degrees celcius.

12. When freezing weather threatens the citrus crop in Florida, growers spray their orange trees with water, using their knowledge of enthalpy to protect the fruit. How much heat is released when 1000 g of liquid water at 10.0°C is completely converted to ice of a temperature of -2.0°C? A. 8.2 x 104 J B: 6.1 x 105 J C. 3.3 x 105 J D.) 3.8 x 10³ J E. 4.2 x 104 J

Calculate the heat change in kilocalories for freezing 265 g of water at 0 ∘C.

The temperature of 34.7 g H2O changes from 27 °C to 53 °C. What is the heat associated with this change? Is heat flowing into or out of the water? How do you know?

When 53.14 grams of fictional compound X is added to water to make 522.1 grams of solution, the temperature increases from 20.89 °C to 64.83 °C. What is the heat of solution for compound X given that the molar mass of compound X is 91.01 g/mol? Assume the specific heat capacity of the solution is 4.18 J/g°C.     164.2 kJ/mol     -164.2 kJ/mol     -95.90 kJ/mol     -11.74 kJ/mol     95.90 kJ/mol

A sample of water at 16.0 °C required an input of 1.97 × 104 J of heat to reach its boiling point, 100.0 °C. What was the mass of the water?

calculate the amount of heat released by 23.0g of water when its temperature is cooled from 68.0'C to 31.0'C. the specific heat of water is 4.18 j/g'c

The heat of fusion of pure silicon is 43.4 kJ/mol. How much energy in kJ would be needed to melt a 6.96-g sample of silicon at its melting point of 1693 K?   Atomic Mass: Si: 28.086 g/mol   Round your answer to 2 decimal places.

4. If a fish caught in a river is placed in a bowl of water and kept in a cool place, it survives for a longer time than when it is in a warm place. Why is this so?