You should use care when dissolving H₂SO4 in water becausethe process is highly exothermic. To measure the enthalpychange, 5.1 g of concentrated H₂SO4(l) was added (withstirring) to 140. g of water in a coffee-cup calorimeter. Thisresulted in an increase in temperature from 21.2 °C to 29.4 °C.Calculate the enthalpy change for the processH₂SO4 (l) → H₂SO4 (aq), in kJ/mol. Assume the specific heatcapacity of the solution is 4.2 J/g. K.Enthalpy changekJ/mol

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You should use care when dissolving H₂SO4 in water because he process is highly exothermic. To measure the enthalpy hange, 5.1 g of concentrated H₂SO4 (l) was added (with tirring) to 140. g of water in a coffee-cup calorimeter. This esulted in an increase in temperature from 21.2 °C to 29.4 °C. Calculate the enthalpy change for the process H₂SO4 (l) – → H₂SO4 (aq), in kJ/mol. Assume the specific heat capacity of the solution is 4.2 J/g. K. Enthalpy change kJ/mol

You should use care when dissolving H₂SO4 in water because he process is highly exothermic. To measure the enthalpy hange, 5.1 g of concentrated H₂SO4 (l) was added (with tirring) to 140. g of water in a coffee-cup calorimeter. This esulted in an increase in temperature from 21.2 °C to 29.4 °C. Calculate the enthalpy change for the process H₂SO4 (l) – → H₂SO4 (aq), in kJ/mol. Assume the specific heat capacity of the solution is 4.2 J/g. K. Enthalpy change kJ/mol

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter4: Energy And Chemical Reactions

Section4.8: Measuring Reaction Enthalpies: Calorimetry

Problem 4.17E

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