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The next three questions pertain to the complete combustion of ethyl acetate under constant pressure: CH3COOC2H5(l) + 5O2(g) 4CO2(g) + 4H2O(l) H =...

The next three questions pertain to the complete combustion of ethyl acetate under constant pressure:
CH3COOC2H5(l) + 5O2(g) ® 4CO2(g) + 4H2O(l) ΔH = -2238.1 kJ/mol
How much heat is given off during the reaction, per mole of water produced?
559.5 kJ/mol

How much heat is given off when 25.6 g of ethyl acetate is burned in excess oxygen?
650. kJ
The burning ethyl acetate from the previous question is used to heat 4.0 L of water at 21.3°C. What would be the final temperature of the water? Assume all the heat produced in the last question is absorbed by the water. Enter your answer in degrees Celsius, without units.

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