The following PEC diagram describes the potential energy and number of configurations of the unmixed state ( UM : AlCl3 (s) + H₂O(1)) and mixed state (M: Al³+ (aq) + 3C1³—(aq)) of aluminum chloride in water. What is true about this ionic compound? Ep Solubility and Temperature Homework Answered a It is soluble at all temperatures с Select an answer and submit. For keyboard navigation, use the up/down arrow keys to select an answer. M It is insoluble at all temperatures UM b It is soluble at low temperatures but insoluble at high temperatures # Config Answered - Incorrect. 1 attempt left d It is soluble at high temperatures but insoluble at low temperatures Resubmit

The following PEC diagram describes the potential energy and number of configurations of the unmixed state ( UM : AlCl3 (s) + H₂O(1)) and mixed state (M: Al³+ (aq) + 3C1³—(aq)) of aluminum chloride in water. What is true about this ionic compound? Ep Solubility and Temperature Homework Answered a It is soluble at all temperatures с Select an answer and submit. For keyboard navigation, use the up/down arrow keys to select an answer. M It is insoluble at all temperatures UM b It is soluble at low temperatures but insoluble at high temperatures # Config Answered - Incorrect. 1 attempt left d It is soluble at high temperatures but insoluble at low temperatures Resubmit

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter9: Energy And Chemistry

Section: Chapter Questions

Problem 9.102PAE: 9.102 A runner generates 418 kJ of energy per kilometer from the cellular oxidation of food. The...

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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.)
Sodium chloride is added in cooking to enhance the flavor of food. When 10.00 g of NaCl are dissolved in 200.0 mL of water at 25.0C in a coffee-cup calorimeter, 669 J of heat are absorbed. (You can make the following assumptions about the solution: volume =200.0 mL, density =1.00 g/mL, specific heat =4.18J/gC) (a) Is the solution process exothermic? (b) What is qH2O? (c) What is the final temperature of the solution?
In a coffee-cup calorimeter, 1.60 g NH4NO3 is mixed with 75.0 g water at an initial temperature of 25.00C. After dissolution of the salt, the final temperature of the calorimeter contents is 23.34C. Assuming the solution has a heat capacity of 4.18 J/C g and assuming no heat loss to the calorimeter, calculate the enthalpy change for the dissolution of NH4NO3 in units of kJ/mol.
In the 1880s, Frederick Trouton noted that the enthalpy of vaporization of 1 mol pure liquid is approximately 88 times the boiling point, Tb, of the liquid on the Kelvin scale. This relationship is called Troutons rule and is represented by the thermochemical equation liquid gas H = 88 Tb, joules Combined with an empirical formula from chemical analysis, Troutons rule can be used to find the molecular formula of a compound, as illustrated here. A compound that contains only carbon and hydrogen is 85.6% C and 14.4% H. Its enthalpy of vaporization is 389 J/g, and it boils at a temperature of 322 K. (a) What is the empirical formula of this compound? (b) Use Troutons rule to calculate the approximate enthalpy or vaporization or one mole of the compound. Combine the enthalpy of vaporization per mole with that same quantity per gram to obtain an approximate molar mass of the compound. (c) Use the results of parts (a) and (b) to find the molecular formula of this compound. Remember that the molecular mass must be exactly a whole-number multiple of the empirical formula mass, so considerable rounding may be needed.
9.102 A runner generates 418 kJ of energy per kilometer from the cellular oxidation of food. The runner's body must dissipate this heat or the body will overheat. Suppose that sweat evaporation is the only important cooling mechanism. If you estimate the enthalpy of evaporation of water as 44 kJ/mol and assume that sweat can he treated as water, describe how you would estimate the volume of sweat that would have to be evaporated if the runner runs a 10-km race.
4. An experiment is to be performed to determine the standard molar enthalpy of neutralization of a strong acid by a strong base. Standard school laboratory equipment and a supply of standardized 1.00 mol/L HCl and standardized 1.00 mol/L NaOH are available. a. What equipment would be needed? List them. b. What measurements should be taken? List them. c. Without performing calculations, briefly describe how the resulting data should be used to obtain the standard molar enthalpy of neutralization. d. When a class of students performed this experiment, the average of the results was -55.0 kJ/mol. The accepted value for the standard molar enthalpy of neutralization of a strong acid by a strong base is -57.7 kilojoules per mole. Briefly describe two likely sources of experimental error that could account for the result obtained by the class. Mistakes, blunders, or miscalculations are not types of experimental error.
Which of the following is FALSE regarding the lab experiment on Calorimetry? a.The specific heat of the calorimeter was calculated in the calibration step. b.The reactions utilized in the calibration step and in the measurement of enthalpy of reaction are both exothermic. c.The enthalpy of reaction for a strong acid-strong base system was calculated in the experiment. d.The ΔHrxn of the reactions used in (1) calibration and (2) in the measurement of ΔHrxn are theoretically equal.
50.0 mL of 1.00 M HCl is mixed with 50.0 mL of 0.95 M KOH in a calorimeter with a caloriemeter constant (K cal ) of 17.3 J/^ C . A change in temperature was observed from 26.0C to 32.6^ ( C. What is the heat of reaction per mole of KOH? (Assume a solution density of 1.00g / (mL) and specific heat capacity of 4.18 J/g^ C .)
A slow heat release pack is to be marketed based on mixing an anhydrous solid with just enough water to form one of its solid hydrates. Which will yield more heat, CaCl2 to CaCl2.6H2O or Na2SO4 to Na2SO4.10H2O? Assume that the same molar quantities of the anhydrous solid are used. You will have to look up the values of ∆H f,m . Sources must be cited appropriately with google
The same student wanted to determine the heat of dissolution for potassium chlorate (KClO3, MW: 122.55 g/mol) in water. He measured 10 grams of KClO3 and dissolved it in a calorimeter containing 250 g of water. The temperature drop was 3.5 K. What is qH2O? What is qrxn? What is ΔHrxn?
The combustion of propane gas leads to formation of carbon dioxide and water by the following equation: C3H8(g) + 5 O2(g) -> 3 CO2(g) + 4 H2O(l) The standard enthalpy for the reaction delta H° = -2220.0 kJ. If 2.84 x 10^3 of kJ of heat are evolved, what volume of CO2 gas in Liters is produced if this reaction occurs at a pressure of 748 tote and 71°C?
To determine the specific heat of a newly created, highly conducting material, a 704.8 mg sample of the material was supplied with 35.548 J of heat causing the temperature of the material to rise from 297.05 K to 461.4 K. What is the specific heat of this material? Report your answer in units of J/(ºC · g) to 4 sig figs, but do NOT include units in your answer.