(8) 9. How much energy is required to heat 81.0 g of water (specific heat = 1.00 cal/g°C) at 11.0°C to steam (specific heat 0.468 cal/g °C) at 123.0°C? (Heat of vaporization of water = 540. cal/g)

The density of liquid oxygen at its boiling point is 1.14 kg/Lkg/L , and its heat of vaporization is 213 kJ/kgkJ/kg . How much energy in joules would be absorbed by 3.0 LL of liquid oxygen as it vaporized? Express your answer to two significant figures and include the appropriate units. ------ Water's heat of fusion is 80. cal/gcal/g , and its specific heat is 1.0calg⋅∘Ccalg⋅∘C . Some velomobile seats have been designed to hold ice packs inside their cushions. If you started a ride with ice packs that held 1300 gg of frozen water at 0 ∘C∘C , and the temperature of the water at the end of the ride was 32 ∘C∘C , how many calories of heat energy were absorbed? Express your answer to two significant figures and include the appropriate units. ---- Water's heat of fusion is 80. cal/gcal/g , its specific heat is 1.0calg⋅∘Ccalg⋅∘C, and its heat of vaporization is 540 cal/gcal/g . A canister is filled with 330 gg of ice and 100. gg of liquid water, both at 0 ∘C∘C . The canister is placed…

Chemistry Using a data below, calculate the molar heat of vaporization of an unknown substance (in units of KB/mol). y=-3125.3×+13.248 andR^2 =0.9375. 1/T,T in Kelvins.

What quantity of heat is required to convert 49 g of ethanol (C₂H₅OH) at 23.0°C to a vapor at 78.3°C (its boiling point)? (heat capacity of ethanol = 2.46 J/g • C; ∆Hvap = 39.3 kJ/mol)