Calculate the amount of heat necessary to change 2.5 kg of ice at 0°C into steam?

Suppose that 0.95 g of steam (aka gaseous water), initially at 100 °C, condenses on a 75.0 g block of iron that is initially at 22 °C. What is the final temperature of the combined system when thermal equilibrium is reached?

What mass of water at 20.0°C must be allowed to come to thermal equilibrium with a 1.95-kg cube of aluminum initially at 150°C to lower the temperature of the aluminum to 60.0°C? Assume any water turned to steam subsequently recondenses. kg

An ice block of mass 1.2000000000000002 kg at an initial temperature of –11 ∘C is put into a copper pot of mass 2.5 kg containing 4.3 L of water at 21 ∘C. If you heat up the pot, what is the amount of energy (in J) you need to convert all the ice and the water into steam? (Assume that no energy is lost from the system.)   You may need some or all of the following constants: The specific heat of ice is 2200 J/kg ∘C, the specific heat of copper is 386 J/kg ∘C and the specific heat of water is 4186 J/kg ∘C. The latent heat of fusion of ice is 334000 J/kg and the heat of vaporization for water is 2256000 J/kg .

What mass of water at 20.0°C must be allowed to come to thermal equilibrium with a 1.90-kg cube of aluminum initially at 150°C to lower the temperature of the aluminum to 70.0°C? Assume any water turned to steam subsequently recondenses. kg

שפיי יוון 6:58 PM | 18.9KB/s ●●● expert.chegg.com/exă Shur 3w/ Question 3 How much heat is required to convert 25.4 g of liquid water (H2O) at 85°C to steam at 135° C? The specific heat capacity for liquid water is 4.18 1/g "C. for steam is 2.01 J/g-C. and the enthalpy of vaporization is 40.7 kJ/mol. Report your answer in kl.

I am stuck on this question i got for homework :( I got a final temperature as 150 degrees Celsius which not possible