[soolee]

Did I do this problem correctly??

If you supply 36 kJ of heat, how many moles of ice at 0 C can be melted, heated to its boiling point, and
completely boiled away? ( H = 40.5 kJ/mol; H = 6.0 kJ/mol; specific heatwater = 0.0753 )

Total heat = heat to melt ice + heat to warm water to 100 C + heat to evaporate water 
Total heat = (moles ice  H ) + (moles water  C T) + (moles water  H ) 
36 kJ = (moles of H O  6.0 kJ/mol) + (moles of H O  0.0753   100 C) + (moles of H O 
40.5 kJ/mol) 
36 kJ = moles H O (6.0 kJ/mol + 0.0753   100 C + 40.5 kJ/mol) 
36 kJ = moles H O (54.0 kJ/mol) 
moles H O =   
moles H O = 0.67 mols??


thank you for your help

[Borek]

Thanks to your use of H and O it is about as obscure as it can be. There is still room for improvement though, you could make it even harder posting in Swahili.

That being said, logic behind what I was able to guess looks correct.