Question

How much energy would need to be input to completely boil 17.3 moles of ice starting at 0 degrees * C and going to 100°C?

(H=40.5 kJ/mol ; H = 6.0kJ / (mol) ; specific

Answer 1

`Q = 934.911\,kJ`

Step-by-step explanation:

The energy needed to boil 17.3 moles of ice is:

`Q = (17.3\,mol)\cdot \left[\left(40.5\,(kJ)/(mol) \right)+ \left((4.186)/(1000)\,(kJ)/(g\cdot ^(\circ)C) \right)\cdot \left((18.015\,g )/(1\,mol) \right)\cdot (100^(\circ)C-0^(\circ)C)+\left(6\,(kJ)/(mol)\right)\right]`
`Q = 934.911\,kJ`