Answer question number one, please. s ar riven at the end of this document.3/28/2021Measurement of Heat Flow & Enthalpy ChangeKCShow the total ionic and net ionic forms of the following equations: If all species are spectator ions, please indicatethat no reaction takes place. Note! You need to make sure the original equation is balanced before proceeding! A setaq)of solubility rules are given at the end of this document.brc1AGNO3(aq) + KC(aq) B AgCl(s) + KNO3(aq)se(2.Mg(NO3)2(aq) + Na2CO3(aq) @ MgCO3(s) + NaNO3(aq)m(3.strontium bromide(aq) + potassium sulfate(aq) l strontium sulfate(s) + potassium bromide(aq)4.manganese(11)chloride(aq) + ammonium carbonate(aq) E manganese(11)carbonate(s) + ammonium chloride(aq)ac5.chromium(1)nitrate(aq) + iron(1)sulfate(aq) l chromium(11)sulfate(aq) + iron(1I)nitrate(aq)Please complete the following reactions, and show the total ionic and net ionic forms of the equation:6.K3PO4(aq) + Al(NO3)3(aq)awiy (Exple velyod fciller7.Belz(aq) + CuzSO4(aq) l8.Ni(NO3)3(aq) + KBr(aq)9.cobalt(11)bromide + potassium sulfide l10.barium nitrate + ammonium phosphate 211.calcium hydroxide + iron(1)chloride l12.rubidium fluoride + copper(1)sulfate lSolubility Rules1. All salts of Group IA, and ammonium are soluble.2 All salts of nitrates, chlorates and acetates are soluble.

GivenAgNO3(aq) + KCl(aq.) →AgCl(s) + KNO3 (aq)Balanced equation = To be determinedNet Ionic Equation…

Show the total ionic and net ionic forms of the following equations. If all species are spectator ions, please indicate that no reaction takes place. Note! You need to make sure the original equation is balanced before proceeding! A set of solubility rules are given at the end of this document. 1AGNO3(aq) + KCl(aq) lAgCl(s) + KNO3(aq)

Show the total ionic and net ionic forms of the following equations. If all species are spectator ions, please indicate that no reaction takes place. Note! You need to make sure the original equation is balanced before proceeding! A set of solubility rules are given at the end of this document. 1AGNO3(aq) + KCl(aq) lAgCl(s) + KNO3(aq)

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter17: Electrochemistry

Section: Chapter Questions

Problem 80AP

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When one mol of KOH is neutralized by sulfuric acid, q=56 kJ. (This is called the heat of neutralization.) At 23.7C, 25.0 mL of 0.475 M H2SO4 is neutralized by 0.613 M KOH in a coffee-cup calorimeter. Assume that the specific heat of all solutions is 4.18J/gC, that the density of all solutions is 1.00 g/mL, and that volumes are additive. (a) How many mL of KOH is required to neutralize H2SO4? (b) What is the final temperature of the solution?
A student followed the procedure in this experiment, using 29.5 mL of 1.59 molar HCl and 31.0 mL of 1.59 molar NaOH, with both solutions having an initial temperature of 22.6 oC. After mixing, a maximum temperature of 33.1 oC is measured. The final mass of the mixture was found to be 64.655 grams. For this problem, assume the specific heat of the solution is 4.18 J/g oC. What is the heat transferred by this reaction, in Joules? Give your answer in in decimal format. When entering units, use proper abbreviated units with proper capitalization.
A student followed the procedure in this experiment, using 29.5 mL of 1.66 molar HCl and 31.5 mL of 1.66 molar NaOH, with both solutions having an initial temperature of 22.1 oC. After mixing, a maximum temperature of 30.7 oC is measured. The final mass of the mixture was found to be 63.194 grams. For this problem, assume the specific heat of the solution is 4.18 J/g oC. What is the heat transferred by this reaction, in Joules? Give your answer in in decimal format.
Determine the standard enthalpy of formation ∆f Hº (in kJ/mol) for HI (g) given that the enthalpy of thereaction 2 HI (g) ---> H2 (g) + I2 (s), is delta H of the reaction = - 53.0 kJmol-1
At constant pressure and 25℃, what is ∆H° for the following reaction 2C2H6 (g)+7O2 (g)→4CO2 (g)+H2O(l) If the complete consumption of 38.2g of C2H6 liberates 1981 kJ of heat energy?
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(a) How much heat is released when 25.0 g of methaneburns in excess O₂ to form gaseous CO₂ and H₂O?(b) Calculate the temperature of the product mixture if themethane and air are both at an initial temperature of 0.0C.Assume a stoichiometric ratio of methane to oxygen from theair, with air being 21% O₂ by volume (c of CO₂=57.2 J/molK;c of H₂O(g)= 36.0 J/molK; c of N=230.5 J/molK).
Chlorodifluoromethane (CHF2Cl) was widely used in the compression/cooling circuits of refrigeration or air-conditioning systems. Since the discovery that such compounds (HCFCs and CFC's) released into the atmosphere were a major cause of depletion of stratospheric ozone, newer refrigeration systems make use of certain hydrofluorocarbons (HFCs), which are degraded in the lower atmosphere, instead. Often, mixtures of such compounds are used. Suppose a sample of refrigerant gas consisting of a simple mixture of the gases pentafluoroethane (C2HF5) and difluorormethane (CH2F2) has a density of 3.06 g/L at 14 °C and 0.974 atm. Calculate the average molecular mass for this sample
Chlorodifluoromethane (CHF2Cl) was widely used in the compression/cooling circuits of refrigeration or air-conditioning systems. Since the discovery that such compounds (HCFCs and CFC's) released into the atmosphere were a major cause of depletion of stratospheric ozone, newer refrigeration systems make use of certain hydrofluorocarbons (HFCs), which are degraded in the lower atmosphere, instead. Often, mixtures of such compounds are used. Suppose a sample of refrigerant gas consisting of a simple mixture of the gases pentafluoroethane (C2HF5) and difluorormethane (CH2F2) has a density of 1.43 g/L at 26 °C and 0.405 atm. Calculate the average molecular mass for this sample. Calculate the volume percentage of CH2F2 in the sample.
Chlorodifluoromethane (CHF2Cl) was widely used in the compression/cooling circuits of refrigeration or air-conditioning systems. Since the discovery that such compounds (HCFCs and CFC's) released into the atmosphere were a major cause of depletion of stratospheric ozone, newer refrigeration systems make use of certain hydrofluorocarbons (HFCs), which are degraded in the lower atmosphere, instead. Often, mixtures of such compounds are used. Suppose a sample of refrigerant gas consisting of a simple mixture of the gases pentafluoroethane (C2HF5) and 111-trifluoroethane (C2H3F3) has a density of 2.39 g/L at 23 °C and 0.593 atm. 1. Calculate the average molecular mass for this sample. 2. Calculate the volume percentage of C2H3F3 in the sample.
Chlorodifluoromethane (CHF2Cl) was widely used in the compression/cooling circuits of refrigeration or air-conditioning systems. Since the discovery that such compounds (HCFCs and CFC's) released into the atmosphere were a major cause of depletion of stratospheric ozone, newer refrigeration systems make use of certain hydrofluorocarbons (HFCs), which are degraded in the lower atmosphere, instead. Often, mixtures of such compounds are used. Suppose a sample of refrigerant gas consisting of a simple mixture of the gases pentafluoroethane (C2HF5) and 111- trifluoroethane ((C2H3F3) has a density of1.95 g/L at 23 °C and 0.432 atm. Calculate the average molecular mass for this sample. Calculate the volume percentage of C2H3F3 in the sample.
Chlorodifluoromethane (CHF2Cl) was widely used in the compression/cooling circuits of refrigeration or air-conditioning systems. Since the discovery that such compounds (HCFCs and CFC's) released into the atmosphere were a major cause of depletion of stratospheric ozone, newer refrigeration systems make use of certain hydrofluorocarbons (HFCs), which are degraded in the lower atmosphere, instead. Often, mixtures of such compounds are used. Suppose a sample of refrigerant gas consisting of a simple mixture of the gases pentafluoroethane (C2HF5) and difluorormethane (CH2F2) has a density of 2.99 g/L at 22 °C and 0.810 atm. Calculate the average molecular mass for this sample.8.94×101 amu Calculate the volume percentage of CH2F2 in the sample.