1. A student wishes to measure the enthalpy change of the reaction of magnesium oxide solid (MgO,M= 40.30 g/mol) with hydrochloric acid (HCI, M= 36.46 g/mol), by the reaction represented in theequation below.MgO(s) +2 HCI(aq)→ MgCL(aq) + H0(E)->(a) Write the net ionic equation for this neutralization reaction.(b) The student designs an experiment to dissolve 1.000 g of Mg0(s) in an insulated cup containing100. g of HCI(aq) with a slight molar excess of the acid. What minimum concentration of HCl inmoles per liter is needed for the experiment? Assume the density of the solution is 1.00 g/mL.(c) The student carries out the experiment and measures a temperature rise of 8.27°C.(i) Assuming the specific heat capacity of the solution is 4.00 J/g °C, calculate the amount ofheat absorbed by the solution from this reaction.(ii) Calculate the experimental enthalpy change for this reaction in J/moln:(iii) The student checks the literature value for AH°.value to be -151 kJ/mol. Caleulate the experimental error the student should report andsuggest at least one possible source of this error.of this reaction and finds the acceptedIxnTxn'(d) The student hypothesizes that using a different strong acid, like perchloric acid (HCIO(aq),M= 100.46 g/mol), will make a significant difference in the enthalpy of the reaction. Doyouagree or disagree with this hypothesis? Justify your answer in terms of net ionic equations.ng or reusing any part of this page is illegal.

We are given mass of MgO = 1g Mass of HCl = 100g Specific heat of solution = 4.00J/g°C…

) Write the net ionic equation for this neutralization reaction. -) The student designs an experiment to dissolve 1.000 g of MgO(s) in an insulated cup conta 100. g of HCI(aq) with a slight molar excess of the acid. What minimum concentration of I moles per liter is needed for the experiment? Assume the density of the solution is 1.00 g/n E) The student carries out the experiment and measures a temperature rise of 8.27°C. (i) Assuming the specific heat capacity of the solution is 4.00 J/g °C, calculate the amou heat absorbed by the solution from this reaction. (ii) Calculate the experimental enthalpy change for this reaction in J/moln

) Write the net ionic equation for this neutralization reaction. -) The student designs an experiment to dissolve 1.000 g of MgO(s) in an insulated cup conta 100. g of HCI(aq) with a slight molar excess of the acid. What minimum concentration of I moles per liter is needed for the experiment? Assume the density of the solution is 1.00 g/n E) The student carries out the experiment and measures a temperature rise of 8.27°C. (i) Assuming the specific heat capacity of the solution is 4.00 J/g °C, calculate the amou heat absorbed by the solution from this reaction. (ii) Calculate the experimental enthalpy change for this reaction in J/moln

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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