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...

See similar textbooks

Similar questions

If 20.0 g of LiOH is added to 0.750 L of 1.00 M Cd(NO₃)₂, how many grams of precipitate will be formed in the following precipitation reaction? a) Write a balanced equation. Identify a precipitate. Include states of matter. b) Determine how much precipitate would form if all reactant 1 ( LiOH) would be used up. c) Determine how much precipitate would form if all reactant 2 ( Cd(NO3 )2 would be used up. d) State Limiting reactant , and theoretical yield ( in grams) of the precipitate that would form from the given amounts.
If all could be answered. Each question can be subtracted from how many questions I have left to ask.
a student separated 7ml of ethyl acetate and butyl acteta via distillation. At the end of the distillation the student obtained 2.7 grams of ethyl acetate. Given that the density of ethly acetate is 0.902g/ml, what is the percent recovery of ethyl acetate
You mix aqueous solutions of 100.0 mL 1.70 M NaCl and 75.o mL 1.20 M Pb(NO3)2, calculate the mass of of precipitate formed.
Solid lead nitrate is slowly added to 125 mL of a 0.0633 M potassium chromate solution. The concentration of lead ion required to just initiate precipitation is M.
Use the table of solubility rules for ionic compounds in water to predict whether each of the following ionic compounds is soluble in water or not using the dropdown on the right. Table of Solubility Rules for lonic Compounds in Water An ionic compound is soluble in water if it contains one of the following: Positive lons: Lit, Na", K*, Rb*, Cs", NH, Negative lons: NO,", C,H,O," CI, Br", I" except when combined with Ag*, Pb2, or Hg, so, except when combined with Ba*, Pb*. Ca, Sr*, or Hg,* 2+ lonic compounds that do not contain at least one of these ions are usually insoluble. Nal [ Choose ] [Choose] soluble in water PbS NOT soluble in water AgCl [ Choose ] LICI [ Choose ] FeO [Choose] KOH [ Choose ]
Q9 solubility products for the following compounds: (a) SrF, 6.3 x 10 g/L, (b) Ag:PO1. 5.7 x 10 From the solubility data given in your Appendix from your textbook, cafculate the PL.
1) What is meaning of the ionization constant and the degree of ionization? And what is the advantage from them? 2) Discusses the graph that practically got it. 3) What is the advantage of using standard solution? And why? And can another solution be used? 4) What is Ostwald's dilution law, and its applications? 5) What happen when the concentration approaches to zero in Ostwald's dilution law? 6) Why did the Arrhenius equation fail to explain the conductivity of concentrated solutions of completely ionized electrolytes? 7) What is the principle of conductivity meter?
1.58g of magnesium hydrogencarbonate was added to a 1.68 mol/L solution of acetic acid, CH3COOH in water (50.0 mL), producing carbon dioxide gas, water and magnesium acetate, Mg(CH3COO)2. a) Write a balanced chemical equation for the reaction. b) What mass of acetic acid is in the aqueous solution? | c) Which of the reactants is the limiting reagent? Justify your answer. d) If 1.23 g of magnesium acetate was produced, what is the percentage yield of the reaction? e) What is the theoretical yield (in grams) of carbon dioxide from this reaction? f) The above reaction is performed in a closed 25 L container at 10 °C. Upon completion of the reaction, what will the final pressure of CO2 be inside the container?
3. When a strip of zinc metal is placed into 1.0 M aqueous FeCl2: (a) nothing happens. (b) chlorine gas forms. (c) iron plates onto the zinc. (d) both (b) and (c) occur.
Discuss the effect of the different preparation on the concentration of the solutions
25 mL of a bleach (NaOCl) sample is diluted to 500 mL. An excessive amount of KI is added to the 20 mL solution taken from here and the I2 released is titrated with 35.5 mL of 0.0409 M NaS2O3. Accordingly, calculate the weight percent by volume of NaOCl in the sample. (MaNaOC:74,4 g/mol)