When 24.0 mL of 0.500 M H2SO4 is added to 24.0 mL of 1.00 M KOH?
2017-10-16 7:12 am
When 24.0 mL of 0.500 M H2SO4 is added to 24.0 mL of 1.00 M KOH in a coffee-cup calorimeter at 23.50°C, the temperature rises to 30.17°C. Calculate ΔH of this reaction. (Assume that the total volume is the sum of the individual volumes and that the density and specific heat capacity of the solution are the same as for pure water.) (d for water = 1.00 g/mL; c for water = 4.184 J/g·°C.)
回答 (2)
2017-10-16 7:51 am
(4.184 J/g·°C) x (24.0 g + 24.0 g) x (30.17 - 23.50)°C = 1339.55 J gained by the water
(1339.55 J) / (0.0240 L x 0.500 mol/L) = 111629 J/mol = 112 kJ/mol
H2SO4 + 2 KOH → K2SO4 + 2 H2O, ΔH = 112 kJ
(1339.55 J) / (0.0240 L x 0.500 mol/L) = 111629 J/mol = 112 kJ/mol
H2SO4 + 2 KOH → K2SO4 + 2 H2O, ΔH = 112 kJ
2017-10-16 7:13 am
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收錄日期: 2021-04-24 00:44:48
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https://hk.answers.yahoo.com/question/index?qid=20171015231253AA7vAEw