Asked by Jen
When 5.00 g of barium hydroxide are added to 250.0 mL of 0.250 hydrochloric acid in a calorimeter, the temperature off the solution increases from 25.0 C to 28.0 C. Calculate the enthalpy ( in kJ per mole of water) given the density of the hydrochloric acid is 1.01 g/mL and the resulting solution is sufficiently dilute that its specific heat is 4.184 J/g C
Answers
Answered by
DrBob222
Ba(OH)2 + 2HCl ==> 2H2O + BaCl2
mols Ba(OH)2 = 5/molar mass = about 0.029 but confirm that.
mols HCl = M x L = about 0.06.
Ba(OH)2 is the limiting reagent and 0.029*2 = mols H2O produced.
q = mass H2O x specific heat H2O x (Tfinal-Tinitial) = ?J
Convert J/(2*0.029 mol H2O) to kJ/mol.
mols Ba(OH)2 = 5/molar mass = about 0.029 but confirm that.
mols HCl = M x L = about 0.06.
Ba(OH)2 is the limiting reagent and 0.029*2 = mols H2O produced.
q = mass H2O x specific heat H2O x (Tfinal-Tinitial) = ?J
Convert J/(2*0.029 mol H2O) to kJ/mol.
There are no AI answers yet. The ability to request AI answers is coming soon!
Submit Your Answer
We prioritize human answers over AI answers.
If you are human, and you can answer this question, please submit your answer.