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

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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