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The density of liquid oxygen at its boiling point is 1.14 kg/L , and its heat...

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Chemistry

The density of liquid oxygen at its boiling point is 1.14 kg/L ,and its heat of vaporization is 213 kJ/kg .

How much energy in joules would be absorbed by 2.0 L of liquidoxygen as it vaporized?

Express your answer to two significant figures andinclude the appropriate units.

Water's heat of fusion is 80. cal/g , and its specific heat is1.0calg??C .

Some velomobile seats have been designed to hold ice packsinside their cushions. If you started a ride with ice packs thatheld 1400 g of frozen water at 0 ?C , and the temperature of thewater at the end of the ride was 32 ?C , how many calories of heatenergy were absorbed?

Express your answer to two significant figures and include theappropriate units.

Water's heat of fusion is 80. cal/g , its specific heat is1.0calg??C, and its heat of vaporization is 540 cal/g .

A canister is filled with 390 g of ice and 100. g of liquidwater, both at 0 ?C . The canister is placed in an oven until allthe H2O has boiled off and the canister is empty. How much energyin calories was absorbed?

Express your answer to two significant figures and include theappropriate units.

Answer & Explanation Solved by verified expert
3.5 Ratings (626 Votes)

1.

mass of oxygen liquid = D*V

                       = 1.14*2 = 2.28 Kg

DHvapourisation = 213 Kj/kg

Amount of heat absorbed = DHvap * m

                        = 213*2.28

                       = 485.64*10^3 joule.

2.


Water's heat of fusion = 80. cal/g

specific heat = 1.0 cal/g⋅∘C .

mass of water = 1400 grams

Heat absorbed (q) = 1400*1*(32-0)+1400*80 = 156800 cal

             = 1.6*10^5 cal


3.
Water heat of fusion = 80. cal/g

specific heat = 1.0 cal/g⋅∘C .

water heat of vaporization = 540 cal/g

Heat absorbed (q) = mice*DHfus + mwater*s*DT + m*DHvap

  
             = 390*80 + (390+100)*1*(100-0)+490*540

             = 3.4*10^5 cal
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