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)

the answer is false because not all countries have geysers under their crust. for example, iceland uses geothermal energy because it is available every in their country.