The heat of neutralization of solid metal hydroxide with an aqueous solution of an acidmight be determined directly in a one-step reactionМОН(s) + H* M'+ H-0(1)or indirectly using a two-step reactionМОН(s) —> М* + онОН + НH2O(1)Based on the net ionic equation of the reaction, the theoretical enthalpy of reaction,AHîheo!liheo kJ/mol], can be found from the enthalpies of formation asΔΗλ ΔΗ; ΗΟ() + ΔΗ Μ' (αq)] -ΔΜΟH (s)]|Based on the measured change in temperature, AT[K], and the heat capacity of the cup,Ccup[J/K], the experimental enthalpy of reaction, AHap[kJ/mol], canfound asAHerp(S„ Viot + Ceup) AT/nL.R.,where Vtot [mL] is the total volume of the solution, nL.R.[mmol] is the amount of thelimiting reagent, and specific heat of water is s, = 4.18 JML¯!K¯lThe percent error can be found according to the formulaAH-AHtheo x 100%%E =expAHiheoUsing the values for standard enthalpies of formation from the table 8-1 find the enthalpiesfor the reactions in the following questions.Question 1Consider two-step neutralization reaction of solid metal hydroxide MOH with anacid. The formation enthalpy of MOH is -438.15 kJ/mol and for Mt it is-249.07 kJ/mol. What is the enthalpy of dissociation?kJ/molWhat is the enthalpy of neutralization of an aqueous solution of solid metal hydroxideMOH with an acid?kJ/mol

The enthalpy of formation of MOH is -438.15 kJ/mol. The formation enthalpy of M+ is -249.07 kJ/mol.

Consider two-step neutralization reaction of solid metal hydroxide MOH with an acid. The formation enthalpy of MOH is -438.15 kJ/mol and for M+ it is -249.07 kJ /mol. What is the enthalpy of dissociation? kJ/mol What is the enthalpy of neutralization of an aqueous solution of solid metal hydroxide MOH with an acid? kJ/mol

Consider two-step neutralization reaction of solid metal hydroxide MOH with an acid. The formation enthalpy of MOH is -438.15 kJ/mol and for M+ it is -249.07 kJ /mol. What is the enthalpy of dissociation? kJ/mol What is the enthalpy of neutralization of an aqueous solution of solid metal hydroxide MOH with an acid? kJ/mol

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter4: Energy And Chemical Reactions

Section: Chapter Questions

Problem 118QRT

See similar textbooks

Similar questions

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?
Benzoic acid, C6H5COOH, is a common standard used in bomb calorimeters, which maintain a constant volume. If 1.20 g of benzoic acid gives off 31, 723 J of energy when burned in the presence of excess oxygen and in a water bath having a temperature of 24.6 C, calculate q, w, H, and U for the reaction.
The enthalpy of combustion of diamond is -395.4 kJ/mol. C s, dia O2 g CO2 g Determine the fH of C s, dia.
A piece of lead of mass 121.6 g was heated by an electrical coil. From the resistance of the coil, the current, and the Time the current flowed, it was calculated that 235 J of heat was added to the lead. The temperature of the lead rose from 20.4C to 35.5C. What is the specific heat of the lead?
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.
Magnesium sulfate is often used in first-aid hot packs, giving off heat when dissolved in water. A coffee-cup calorimeter at 25C contains 15.0 mL of water at 25C. A 2.00-g sample of MgSO4 is dissolved in the water and 1.51 kJ of heat are evolved. (You can make the following assumptions about the solution: volume=15.0 mL, density=1.00 g/mL, specific heat=4.18J/gC.) (a) Write a balanced equation for the solution process. (b) Is the process exothermic? (c) What is qH2O? (d) What is the final temperature of the solution? (e) What are the initial and final temperatures in F?
Write reactions for which the enthalpy change will be a. Hf for solid aluminum oxide. b. the standard enthalpy of combustion of liquid ethanol, C2H5OH(l). c. the standard enthalpy of neutralization of sodium hydroxide solution by hydrochloric acid. d. Hf for gaseous vinyl chloride, C2H3Cl(g). e. the enthalpy of combustion of liquid benzene, C6H6(l). f. the enthalpy of solution of solid ammonium bromide.
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.
One step in the manufacturing of sulfuric acid is the conversion of SO2(g) to SO3(g). The thermochemical equation for this process is SO2(g)+12O2(g)SO3(g)H=98.9kJ The second step combines the SO3 with H2O to make H2SO4. (a) Calculate the enthalpy change that accompanies the reaction to make 1.00 kg SO3(g). (b) Is heat absorbed or released in this process?
Would the amount of heat absorbed by the dissolution in Example 5.6 appear greater, lesser, or remain the same if the heat capacity of the calorimeter were taken into account? Explain your answer.