Question
In: Chemistry
50.0 mL of 1.00 M of a solution of HCl at 18.0 ºC is combined with...
50.0 mL of 1.00 M of a solution of HCl at 18.0 ºC is
combined with 50.0 mL of 1.00 M solution of NaOH at 18.0 ºC. The
final temperature of the reaction mixture is 24.6 ºC. If the heat
capacities and densities of these solutions are approximately the
same as water (4.184 J/g · ºC, 1.00 g/mL), what is the molar heat
of neutralization (∆Hneut.)? Is this reaction endothermic or
exothermic? [2 pt.]
HCl (aq) + NaOH (aq) → NaCl (aq) + H2O (l)
Solutions
Expert Solution
No of mole of HCl = 50*1/1000 = 0.05 mole
No of mole of NaOH = 50*1/1000 = 0.05 mole
total mass of mixture = d*V
= (50+50)*1 = 100 g
heat released in the reaction(q) = m*s*DT
= 100*4.184*(24.6-18)
= 2.7614 kj
enthalpy of neutralisation(DH0neu) = 2.7614 kj/0.05 mole
= 55.23 kj/mol
as temperature increases, it is exothermic process
queen_honey_blossom answered 2 years agoRelated Solutions
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