What amount of energy is required to melt a 10.7 g piece of ice at 0 C? The heat of fusion of ice = 333 Jg-1

Answer 1

Approx. #3.5*kJ#...........Why?

We carry out the bodily response.

#H_2O(s) +Deltararr H_2O(l)#; both reactants and products are at #0# #""^@C#, and thus we need only assess the energy transfer of the PHASE change........
We are given the #"heat of fusion"# of ice in #J*g^-1#....
We gots a #10.7*g# mass of ice, and so we take the product.........
#10.7*cancelgxx333*J*cancel(g^-1)xx10^-3*J*kJ^-1=??J#....
And this represents HEAT, #Delta#, put into the system.........is the sign correct?
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Answer 2

The amount of energy required to melt a 10.7 g piece of ice at 0°C is:

( Q = m \times \text{heat of fusion} )

( Q = 10.7 , \text{g} \times 333 , \text{J/g} )

( Q = 3563.1 , \text{J} )

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Answer from HIX Tutor

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

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