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What quantity of heat (in kJ) would be required to convert 15.1 g of ice to water at 0.00°C? (∆Hfus = 6.01 kJ/mol for water)
for the answer I got 5.04, I don't know if it is correct
if it's correct, how would the process change if celsius was not zero, or does nothing change.

Respuesta :

onyebuchinnaji

The quantity of heat required to convert the ice to water is 5048.4 J.

Quantity of heat required

The quantity of heat required to convert the ice to water is calculated as follows;

Q = n∆Hfus

where;

  • n is the number of moles of the ice
  • ∆Hfus is heat of fusion = 6.01 kJ/mol

Number of moles of the ice

The number of moles of the ice is calculated as follows;

n = m/M

where;

M is molar mass of water (H2O) = 18 g/mol

n = 15.1/18

n = 0.84 mole

Q = 0.84 x 6.01 x 10³

Q = 5048.4 J

Thus, the quantity of heat required to convert the ice to water is 5048.4 J.

Learn more about quantity of heat here: https://brainly.com/question/13439286

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