(l) ∆H H++ = 0, ∆H OH−− = -230 kJ/mol, ∆H H2O = -286 kJ/mol ∆H reactants = ∆H H++ + ∆H OH−− = -230 + 0 = -230 kJ/mol ∆H reactants = -286 kJ/mol - ( -230 kJ/mol) = -56 kJ/mol predict the final temperature by solving for ∆T in the equation,assume the solution has approximately the same density as water, 1.00g/mL.
(l) ∆H H++ = 0, ∆H OH−− = -230 kJ/mol, ∆H H2O = -286 kJ/mol ∆H reactants = ∆H H++ + ∆H OH−− = -230 + 0 = -230 kJ/mol ∆H reactants = -286 kJ/mol - ( -230 kJ/mol) = -56 kJ/mol predict the final temperature by solving for ∆T in the equation,assume the solution has approximately the same density as water, 1.00g/mL.
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Initial temp: 19.06 C
0.5 M concentration 200 mL of HCl and 200 mL of NaOH are combined in an insulated container.
H++ (aq) + OH−− (aq) - - -> H2O (l)
H+(aq) + OH-(aq) - - -> H2O (l)
∆H H++ = 0, ∆H OH−− = -230 kJ/mol, ∆H H2O = -286 kJ/mol
∆H reactants = ∆H H++ + ∆H OH−−
= -230 + 0
= -230 kJ/mol
∆H reactants = -286 kJ/mol - ( -230 kJ/mol)
= -56 kJ/mol
predict the final temperature by solving for ∆T in the equation,assume the solution has approximately the same density as water, 1.00g/mL.
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