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.

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)

b is the correct answer

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