Calculate the total energy required to change 22 g of ice at - 20 degrees Celsius, to water, with a temperature of 50 degrees Celsius. The heat capacity of ice is 2.03 J/g-C, the heat capacity of water is 4.184 J/g-C, and the molar heat of fusion for ice is 6.02 kJ/mol.

Question

Tippy

Chemistry

14 August, 07:40

Calculate the total energy required to change 22 g of ice at - 20 degrees Celsius, to water, with a temperature of 50 degrees Celsius. The heat capacity of ice is 2.03 J/g-C, the heat capacity of water is 4.184 J/g-C, and the molar heat of fusion for ice is 6.02 kJ/mol.

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Vernon · Answer 1

q (total) needed = 140Kj (2 sig. figs. based on mass of ice)

Explanation:

Total Energy = ∑phase transition energies = ∑q = q (heating ice) + q (melting ice) + q (warming water to 50°C)

q (total) = mcΔT (warming ice) + mΔH (melting ice) + mcΔT (warming water)

= [ (22g) (2.03j/g·°C) (20°C) ]warming ice + [ (22g) (6020j/g) ]melting ice + [ (22g) (4.184j/g·°C) (50°C) ]warming water

= (893.2j) warming ice + (132,440j) melting ice + (46,024j) warming water

= 137,935.6joules = 138Kj ≅ 140Kj (2 sig. figs. based on mass of ice)