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 in an oven until all the H2OH2O has boiled off and the canister is empty. How much energy in calories was absorbed? Express your answer to two significant figures and include the appropriate units.

A 135.0 L weather balloon filled with 6.40 mol of helium has a small leak. If the helium leaks at a rate of 10.0 mmol/hr, what is the volume of the balloon after 69.0 hours? L

Use the following values to answer each part. The specifi c heat of water is 1.00 cal/(g · °C); the heat of fusion of water is 79.7 cal/g; and the heat of vaporization of water is 540 cal/g. a. How much energy (in calories) is needed to melt 45 g of ice at 0.0 °C and warm it to 55 °C? b. How much energy (in calories) is released when 45 g of water at 55 °C is cooled to 0.0 °C, and frozen to solid ice at 0.0 °C? c. How much energy (in kilocalories) is released when 35 g of steam at 100. °C is condensed to water, the water is cooled to 0.0 °C, and the water is frozen to solid ice at 0.0 °C?

Ethanol (C₂H₂OH) meits at-114 °C and boils at 78°C. The enthalpy of fusion of ethanol is 5.02 kJ/mol, and its enthalpy of vaporization is 38.56 kJ/mol. The specific heat of solid and liquid ethanol are 0.97 and 2.3 J/(g-K), respectively. Y Part A How much heat is required to convert 30.5 g of ethanol at 28 °C to the vapor phase at 78 "C? Express your answer in kilojoules to three significant figures. 195] ΑΣΦ Submit Part 8 Request Answer Submit ? How much heat is required to convert 30.5 g of ethanol at-160 C to the vapor phase at 78 "C7 Express your answer in kilojoules to two significant figures. VA24 Request Answer kJ kJ

Ethanol (C2 H5 OH) melts at -114 °C. The enthalpy of fusion is 5.02 kJ/mol. The specific heats of solid and liquid ethanol are 0.97 J/g-K and 2.3 J/g-K, respectively. How much heat (kJ) is needed to convert 25.0 g of solid ethanol at -125 °C to liquid ethanol at -50 °C? 3949 207.3 6.67 8.97 -12.5

Calculate the energy (in kcal) required to convert one ice cube that was made by freezing 72 mL of water (density = 1.000 g/L) an an initial temperature of -36.0 C, to liquid water at a final temperature of 37.0 CH2O(s) --> H2O(l) ΔH = +6.02 kj/mol Cpm H2O(s) = 37.7 J/mol x K  Cpm H2O(l) = 75.4 J/mol x K  1 kcal = 4.18 kJ

What quantity of heat, in kJ, is required to convert 12.0 g of ethanol (C₂H₂OH) at 23.0°C to a vapor at 78.3°C (its boiling point)? (specific heat capacity of ethanol = 2.46 J/g C; AHvap = 39.3 kJ/mol) ●

How much heat energy is required to convert 77.6 g of solid iron at 21 °C to liquid iron at 1538 °C? The molar heat of fusion of iron is 13.8 kJ/mol. Iron has a normal melting point of 1538 °C. The specific heat capacity of solid iron is 0.449 J/(g · °C). q= kJ