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6 Nov 2019
A 100.0mL solution of 1.05 H2SO4 at 23.2degrees Celcius is mixed with 100.0mL of 2.0 M NaOH, also at 23.2degrees Celcius, in a coffee-cup calorimeter. After the reactionoccurs, the temperature of the resulting mixture is 35.7 degreesCelcius. The density of the final solution is 1.06g/mL. Calculatethe molar heat of neutralization. Assume the specific heat of thesolution is 4.184 J/g*C. The heat capacity of the calorimeter is32.5 J/C.
(1/2)H2SO4 (aq) + NaOH(aq) =>(1/2)Na2SO4 (aq) + H2O(l)
a. 41.7 kJ/mol
b. 57.5 kJ/mol
c. 45.9 kJ/mol
d. 13.0 kJ/mol
e. 33.9 kJ/mol
A 100.0mL solution of 1.05 H2SO4 at 23.2degrees Celcius is mixed with 100.0mL of 2.0 M NaOH, also at 23.2degrees Celcius, in a coffee-cup calorimeter. After the reactionoccurs, the temperature of the resulting mixture is 35.7 degreesCelcius. The density of the final solution is 1.06g/mL. Calculatethe molar heat of neutralization. Assume the specific heat of thesolution is 4.184 J/g*C. The heat capacity of the calorimeter is32.5 J/C.
(1/2)H2SO4 (aq) + NaOH(aq) =>(1/2)Na2SO4 (aq) + H2O(l)
a. 41.7 kJ/mol
b. 57.5 kJ/mol
c. 45.9 kJ/mol
d. 13.0 kJ/mol
e. 33.9 kJ/mol
homerun2015Lv7
27 Mar 2023
Elin HesselLv2
26 Oct 2019
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