a chemist mixes 30.0ml of 1.50M phosphoric acid, H3PO4, with 50.0mL of 1.50M NaOH in a coffee cup calorimeter. The following reaction occurs: H3PO4 + 3OH- = 3H2O + PO4-3. The temperature in the calorimeter rises from 21.00 to 24.76. Find the delta H for the neutralization reaction as written in the balanced equation shown above. The density of the solution is 0.9882g/ml and the specific heat capacity of the solution is 4.18j/g C
a chemist mixes 30.0ml of 1.50M phosphoric acid, H3PO4, with 50.0mL of 1.50M NaOH in a coffee cup calorimeter. The following reaction occurs: H3PO4 + 3OH- = 3H2O + PO4-3. The temperature in the calorimeter rises from 21.00 to 24.76. Find the delta H for the neutralization reaction as written in the balanced equation shown above. The density of the solution is 0.9882g/ml and the specific heat capacity of the solution is 4.18j/g C
Introduction to Chemical Engineering Thermodynamics
8th Edition
ISBN:9781259696527
Author:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Publisher:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Chapter1: Introduction
Section: Chapter Questions
Problem 1.1P
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a chemist mixes 30.0ml of 1.50M phosphoric acid, H3PO4, with 50.0mL of 1.50M NaOH in a coffee cup calorimeter. The following reaction occurs: H3PO4 + 3OH- = 3H2O + PO4-3. The temperature in the calorimeter rises from 21.00 to 24.76.
Find the delta H for the neutralization reaction as written in the balanced equation shown above.
The density of the solution is 0.9882g/ml and the specific heat capacity of the solution is 4.18j/g C
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