25.0 kJ of heat is added to 52.0g of ice at -10.0°C. What is the temperature of the water (in °C that forms. specific heat of ice: 2.09 J/g-°C AHfus = 6.02 kJ/mol specific heat of water: 4.18 Jig-°C AHvap = 40.7 kJ/mol specific heat of steam: 2.00 J/g.°C Express your answer in decimal notation rounded to TWO significant figures.

How much heat (in kJ) is required to warm 64.8 grams of ice to steam? The ice starts at an initial temperature of -16.2 °C and is warmed to steam at 107.5 °C. The heat capacities are: Cice = 2.09 J/g.°C Cwater = 4.184 J/g°C Csteam = 2.01 J/g°C The heat of fusion is 6.02 kJ/mol The heat of vaporization is 40.7 kJ/mol

A 5.00 g sample of water vapor, initially at 155*C is cooled at atmospheric pressure, producing ice at -55*C. Calculate the amount of heat energy lost by the water vapor sample in this process, in kJ. Use the following data specific heat capacity of ice is 2.09 J/ gK; the specific heat capacity of liquid water is 4.18 J/ gK; the specific heat capacity of water vapor is 1.84 J/ gK; the heat of fusion of ice is 336 J/g; the heat of vaporization of water is 2260 J/g. ( I know the answer is 15.6 kJ but I don't know how to get to it, Pls help ASAP!!)show all the steps you can pls

How many joules of heat energy are needed to heat 25.0 g of ice at -5.0°C to a final temperature of 40.0°C. Specific heat of ice = 2.1 J/g°C. Be sure to consider the state of H20 present at 40.0°C.

If we start with 10g of ice at -5°C and heat it until we have liquid water at 45°C, how much heat energy will be needed (kJ)?     The specific heat of ice is 2.03J/g°C and the specific heat of liquid water is 4.18J/g°C.     ΔHfusion is 334 J/g.

A total of 537 cal of heat is added to 5.00 g of ice at -20.0 °C. What is the final temperature of the water? Tfinal = °C Specific heat of H₂O(s) Specific heat of H₂O(l) Heat of fusion for H₂O 2 2.087 J/(g. °C) 4.184 J/(g. °C) 333.6 J/g

1. Calculate the amount of heat that must be absorbed by 10.0 gram of ice at -20C to convert it to liquid water at 60.0C. Given: Specific heat (ice) = 2.1 J/g.C Specific heat (water) = 4.18 J/g-C Hfus = 6.0 kJ/mol or 334 J/g

What amount of heat must be added to melt 54.06 g of ice at 0 °C and increase the temperature to 22.0 °C? Specific heats: ice 2.108 , water 4.184- g.°C steam 1.996 g°C heat of fusion for water 6.01 kJ/mol, heat of vaporization for water 40.65 kJ/mol

Calculate the total amount of heat released when 40.5 g of water at 85.0°C is converted to ice at -30.0 °C. (Hfus at 0 °C = 6.01 kJ/mol; specific heat of water = 4.18 J/g-°C; specific heat of ice = 2.09 J/g-°C)