Calculation of standard molar enthalpiesData:Standard molar enthalpy of formation of H2O (g): AƒH°1 = -241.6 kJ mol-1Standard molar enthalpy of formation of H2O2 (g): AfH°2= -140.4 kJ mol-'Standard molar enthalpies of bond dissociation:AdissH°(H2(g)) = 435.6 kJ mol-'; AdissH°(O2(g)) = 497.8 kJ mol-!Calculate:AdissH°(O-O) or D(O-O), the standard molar enthalpy of dissociation of the O-O bond in themolecule of hydrogen peroxide H2O2 of structural formula H-O-0-H. The dissociationenthalpy of the O-H bond in H2O and in H2O2 will be considered as equal.

Bond dissociation enthalpy is the enthalpy change associated with the process in which 1 mol of…

Answered: Standard molar enthalpy of formation of…

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 96QRT

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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.
For the process A(l) A(g), which direction is favored by changes in energy probability? Positional probability? Explain your answers. If you wanted to favor the process as written, would you raise or lower the temperature of the system? Explain.
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.
at if Hess’s law were not true? What are some possible repercussions this would have?
When 1.000 g of ethylene glycol, C2H6O2, is burned at 25C and 1.00 atmosphere pressure, H2O(l) and CO2(g) are formed with the evolution of 19.18 kJ of heat. a Calculate the molar enthalpy of formation of ethylene glycol. (It will be necessary to use data from Appendix C.) b Gf of ethylene glycol is 322.5 kJ/mol. What is G for the combustion of 1 mol ethylene glycol? c What is S for the combustion of 1 mol ethylene glycol?
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.
2.8 g of a solid was dissolved in 51.4 g of a basic solution in a calorimeter with a calorimeter constant of 37.0 J K–1 with all substances initially at 81.5 °C.The resulting solution was observed to be at a temperature of 59.8 °C and have a heat capacity of 3.81 J g–1 K–1.Determine q for the dissolution process.
Consider the following reaction: H2(g) + ½ O2 (g) ------> H2O (g) The standard enthalpy of formation of gaseous H2O at 298 K is -241.82 kJ mol-1. Calculate the value at 153 0C. Given Cp,m for H2O(g): 33.58 kJ mol-1; H2 (g): 28.84 kJ mol-1; O2 (g): 29.37 kJ mol-1. Assume heat capacities are independent of T. NOTE:answer in kilojoules per mole (kJ/mol)
At constant pressure and 25C, what is enthalpy for the reaction: 2C2H6 + 7O2 -> 4CO2 + H2O, if the complete consumption of 12g of C2H6 liberates - 700kJ of heat energy? (-3508 kJ)
Benzoic acid of mass 1.40 g is reacted with oxygen in a constant volume calorimeter to form H2O(l) and CO2(g) at 298 K. The mass of the water in the inner bath is 1.40×103g. The temperature of the calorimeter and its contents rises 2.84 K as a result of this reaction. Part A Calculate the calorimeter constant. The standard enthalpy of combustion of benzoic acid at 298 K is −3227 kJ⋅mol−1. CP,m(H2O,l)=75.3J⋅mol−1⋅K−1.
A sample of the sugar d-ribose (C5H10O5) of mass 0.727 g was placed in a calorimeter and then ignited in the presence of excess oxygen. The temperature rose by 0.910 K. In a separate experiment in the same calorimeter, the combustion of 0.825 g of benzoic acid, for which the internal energy of combustion is −3251 kJ mol−1, gave a temperature rise of 1.940 K. Calculate the enthalpy of formation of d-ribose.
The standard enthalpy of formation of H2O(l) at 298 K is -285.8 kJ/mol.Calculate the change in internal energy for the following process at 298 K and 1 atm: H2O (l) → H2 (g) + 1/2 O2 (g) ΔE° = ?

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