Answer question number six, please. Also, I would like the work wrote out if you can. Thanks so much I truly appreciate it. AgCI(S)3/28/2021Measurement of Heat Flow & Enthalpy ChangeShow 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 setof solubility rules are given at the end of this document.1AGNO3(aq) + KCl(aq) AgCl(s) + KNO3(aq)2.Mg(NO3)2(aq) + Na2CO3(aq) l MgCO3(s) + NANO3(aq)3.strontium bromide(aq) + potassium sulfate(aq) l strontium sulfate(s) + potassium bromide(aq)4.manganese(11)chloride(aq) + ammonium carbonate(aq) 2 manganese(11)carbonate(s) + ammonium chloride(aq)5.chromium(111)nitrate(aq) + iron(11)sulfate(aq) chromium(111)sulfate(aq) + iron(11)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) ®your thess od fose el, kogic7.Belz(aq) + CuzSO4(aq) @8.Ni(NO3)3(aq) + KBr(aq) l9.cobalt(111)bromide + potassium sulfide larces the10.barium nitrate + ammonium phosphate l11.calcium hydroxide + iron(1II)chloride l12.rubidium fluoride + copper(1I)sulfate lSolubility Rules1. All salts of Group IA, and ammonium are soluble.2. All salts of nitrates, chlorates and acetates are soluble.3. All salts of halides are soluble except those of silver(1), copper(), lead(11), and mercury().4 All salts of sulfate are soluble except for barium sulfate, lead(1) sulfate, and strontium sulfate.5 All salts of carbonate, phosphate and sulfite are insoluble, except for those of group IA and ammoniu

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Answered: 6.K3PO4(aq) + Al(NO3)3(aq)

Science

Chemistry

6.K3PO4(aq) + Al(NO3)3(aq)

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter8: Thermochemistry

Section: Chapter Questions

Problem 12QAP: The heat of neutralization, Hneut, can be defined as the amount of heat released (or absorbed), q,...

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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?
The heat of neutralization, Hneut, can be defined as the amount of heat released (or absorbed), q, per mole of acid (or base) neutralized. Hneut for nitric acid is -52 kJ/mol HNO3. At 27.3C, 50.00 mL of 0.743M HNO3 is neutralized by 1.00 M Sr(OH)2 in a coffee-cup calorimeter. (a) How many mL of Sr(OH)2 were used in the neutralization? (b) What is the final temperature of the resulting solution? (Use the assumptions in Question 11.)
A coffee-cup (constant pressure) calorimeter is used to carry out the following reaction in 63.5 mL water (where X is a hypothetical metal): X + 2 HCl → XCl2 + H2 In this process, the water temperature rose from 25.0 °C to 34.1 °C. If 0.00618 mol of "X" was consumed during the reaction, what is ΔrH of this reaction in kJ mol-1 with respect to "X"? The specific heat of water is 4.184 J g-1 °C-1 Express in 2 sig digs!
A student dissolves13.7 g of sodium chloride NaCl in 250.g of water in a well-insulated open cup. She then observes the temperature of the water fall from 23.0°C to 21.4°C over the course of 4.5 minutes. Use this data, and any information you need from the ALEKS Data resource, to answer the questions below about this reaction: NaCls -> Na+aq + Cl−aq You can make any reasonable assumptions about the physical properties of the solution. Be sure answers you calculate using measured data are rounded to the correct number of significant digits. Is this reaction exothermic, endothermic, or neither? If you said the reaction was exothermic or endothermic, calculate the amount of heat that was released or absorbed by the reaction in this case. Calculate the reaction enthalpy ΔHrxn per mole of NaCl.
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.
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 volume percentage of CH2F2 in the sample.
A coffee cup calorimeter with a heat capacity of 4.90 J/∘C was used to measure the change in enthalpy of a precipitation reaction. A 50.0 mL solution of 0.360 M AgNO3 was mixed with 50.0 mL of 0.480 M KCl. After mixing, the temperature was observed to increase by 2.80∘C.Calculate the enthalpy of reaction, Δ?rxn, per mole of precipitate formed (AgCl). Assume the specific heat of the product solution is 4.17 J / (g⋅∘C) and that the density of both the reactant solutions is 1.00 g/mL. Calculate the theoretical moles of precipitate formed from AgNO3 and KCl. Calculate the heat change experienced by the calorimeter contents, ?contents. Calculate the heat change experienced by the calorimeter, ?cal. Calculate the heat change produced by the solution process, ?solution. Calulate Δ?solution for one mole of precipitate formed. I'm just going to go ahead and say thank you to whoever decides to answer this question. I really appreciate the help I have received. ?