Answer to Question #169410 in General Chemistry for Dawson

Question #169410

When 28.2 mL of 0.500 M H2SO4 is added to 28.2 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.). Do not answer in scientific notation.

1
Expert's answer
2021-03-10T06:05:41-0500

H2SO4 + 2NaOH = Na2SO4 + H2O.

28.2 x 0.5/1000 = 0,0141 moles of Na2SO4. and 2,0022 g.

Q=mc∆T = 2,0022 x 4.184 x 6,97 = 58,3891175 J.


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