If you have 10 grams of ice at -11 degrees celsius, find the energy it takes to turn it into water.

If you have 10 grams of ice at -11 degrees celsius, find the energy it takes...
Compute the total thermal energy required to convert 0.030 grams of ice at -20 degrees Celsius to warm water at 60 degrees Celsius.
20 grams of ice at -12 degrees celsius is added to 300 grams of water at 30 degrees celsius. When equilibrium is reached, what is the temperature in celsius of the water?
You have 400.0 grams of room temperature water at 20.0 degrees Celsius in a thermos flask. You drop 130.0 grams of ice at 0.00 degrees Celsius into the thermos and shut the lid. (a) What is the equilibrium temperature of the system? (b) How much ice is left in grams? Answer up to 3 significant figures.
155 grams of ice at -10.0 degrees celsius is added to 1.17 kg of water at 70.0 degrees celsius and mixed together in thermal isolation until they come to equilibrium. The specific heat of ice is 2010 J/kgC. The specific heat of water is 4186 J/kgC. The latent heat of fusion for water is 3.34x10^5 J/kg. The latent of vaporization for water is 2.26x10^6 J/kg. What is the final equilibrium. The answer is 51.9 celsius. I just need the steps...
How much heat is needed to convert 200 grams of ice at 0 degrees Celsius to steam at 100 degrees Celsius?(Hf(0 C)=334 J/g, Specific heat of water = 4.184 J/gK, Hv(100 C) = 2260 J/g, Specific heat of ice = 2.108 J/gC) and how do i do it?
A 50g ice cube is taken out of a freezer at 0 degrees Celsius and put in a thermally isolated container containing 200g of water at the temperature 60 degrees Celsius. Find the temperature of the system at equilibrium. ANSWER: 32 degrees Celsius I don't understand why you have to involve (moles of ice x delta H of fusion) to the equation? Please help! Thanks!
How many grams of ice at -24.9 degrees Celsius can be completely converted to liquid at 5.1 degrees Celsius if the available heat for this process is 4.22x10^3 kJ? For ice, use a specific heat of 2.01J/(gxC) and enthalpy of fusion of 6.01kJ/mol.
How many grams of ice at -24.9 degrees Celsius can be completely converted to liquid at 5.1 degrees Celsius if the available heat for this process is 4.22x10^3 kJ? For ice, use a specific heat of 2.01J/(gxC) and enthalpy of fusion of 6.01 kJ/mol.
How much heat is required to heat 25 g of ice at -10 degrees Celsius to water vapor at 100 degrees Celsius. Specific heat (ice) = 2.10 J/degree Celsius Specific Heat (water) = 4.18 J/degree Celsius Heat of fusion = 333 J/g Heat of Vaporization = 2258 J/g
if 65g of ice at 0.0 degrees celsius is placed in 245mL of water at 35 degrees celsius, find the final temperature if all of the ice melts. STEP BY STEP PLEASE