Fusion and vaporization please help

five stars to whoever does these first

1. Ice has a specific heat of 2.1 J/gCo. How much heat would be needed to raise the temperature of 403.0 grams of ice from minus 25oC to zero oC?

2.How much heat (in joules) is required to change the 403.0 grams of ice at zero oC to water at zero oC? Remember that the heat of fusion for water is 6.01 kJ/mol. Note that this is kilojoules/mol not J/mol.

3.How much heat is needed to raise the temperature of 403.0 grams of water from zero oC to 100 oC? The specific heat of water is 4.18 J/gCo

4.How much heat (in joules) is required to convert 403.0 grams of water at 100oC to steam at 100oC? The heat of vaporization for water is 40.7 kJ/mol. Note again that this is kilojoules/mol not joules/mol

5.How much heat is required to raise the temperature of 403.0 grams of steam at 100 oC to steam at 122oC? The specific heat of steam is 1.7 J/gCo.

6.At this point, we should be able to determine the total heat required to raise the temperature of 403.0 grams of ice from minus 25oC to steam at 22oC. Just find the sum of all the answers above

all answers need to be in joules thank you in advance

1. Heat = mass of substance x specific heat capacity x change in temperature.
Heat = (403.0 g)(2.1 J/gCo)[0 - (-25)]Co = 2.12 x 10^4 J.

2. Heat of phase change = +- moles of substance x molar heat of phase change.
Moles ice = mass/molar mass = 403.0 g/(18.016 g/mol) = 22.37 mol, so
Heat = (22.37 mol)(6.01 kJ/mol) = 134.4 kJ = 1.34 x 10^5 J.

Note: positive sign is used for when substance undergoing phase absorbs heat, negative sign
when it releases heat or heat is removed from it.

3. Use the same formula stated in 1.
Heat = (403.0 g)(4.18 J/gCo)(100 - 0)Co = 1.68 x 10^5 J.

4. Use same formula stated in 2.
Heat = (22.37 mol)(40.7 kJ/mol) = 910.4 kJ = 9.10 x 10^5 J.

5. Heat = (403.0 g)(1.7 J/gCo)(122 - 100)Co = 1.507 x 10^4 J.

6. [(2.12 x 10^4) + (1.34 x 10^5) + (1.68 x 10^5) + (9.10 x 10^5) + (1.507 x 10%