When 0.243 g of Mg metal is combined with enough HCl tomake 100 mL of solution in a constant-pressure calorimeter,the following reaction occurs:Mg1s2 + 2 HCl1aq2¡MgCl21aq2 + H21g2If the temperature of the solution increases from 23.0 to34.1 °C as a result of this reaction, calculate ΔH in kJ>mol Mg.Assume that the solution has a specific heat of 4.18 J>g@°C anda density of 1.00 g/mL. (a) -19.1 kJ>mol (b) -111 kJ>mol(c) -191 kJ>mol (d) -464 kJ>mol (e) -961 kJ>mol
When 0.243 g of Mg metal is combined with enough HCl tomake 100 mL of solution in a constant-pressure calorimeter,the following reaction occurs:Mg1s2 + 2 HCl1aq2¡MgCl21aq2 + H21g2If the temperature of the solution increases from 23.0 to34.1 °C as a result of this reaction, calculate ΔH in kJ>mol Mg.Assume that the solution has a specific heat of 4.18 J>g@°C anda density of 1.00 g/mL. (a) -19.1 kJ>mol (b) -111 kJ>mol(c) -191 kJ>mol (d) -464 kJ>mol (e) -961 kJ>mol
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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When 0.243 g of Mg metal is combined with enough HCl to
make 100 mL of solution in a constant-pressure calorimeter,
the following reaction occurs:
Mg1s2 + 2 HCl1aq2¡MgCl21aq2 + H21g2
If the temperature of the solution increases from 23.0 to
34.1 °C as a result of this reaction, calculate ΔH in kJ>mol Mg.
Assume that the solution has a specific heat of 4.18 J>g@°C anda density of 1.00 g/mL. (a) -19.1 kJ>mol (b) -111 kJ>mol
(c) -191 kJ>mol (d) -464 kJ>mol (e) -961 kJ>mol
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