The standard enthalpies of formation of ions in aqueous solution are obtained by arbitrarilyassigning a value of zero to H* ions; that is A,H° | H* (aq) =0.(a) If A,H° [HCI(g)]=-92.3 kJ mol', calculate A,H° | cI" (aq)| for the following reaction,-1HCl(g) → H*(aq) + Cl (aq)A,H° = –74.9 kJ mol(b) If A,H° | H,O(1)|=-285.8 kJ mol", calculate A,H°|OH (aq) for the following reaction,1Н (аq) +ОН (аq)—> H2О()4,H° =-56.2 kJ mol-

(a) The given data is as follows: HCl(g) → H+(aq) + Cl-(aq) ∆rH=-74.9 kJ mol-1…

The standard enthalpies of formation of ions in aqueous solution are obtained by arbitrarily assigning a value of zero to H* ions; that is A,H° H (aq)|=0. (a) If A,H° [HC1(g)]=-92.3 kJ mol", calculate A, H[CI (ag)] for the following reaction, HCI(g) → H*(aq) + CI (aq) A,H° = -74.9 kJ mol (b) If A,H° [H,0(1)] =-285.8 kJ mol", calculate A,H° OH (aq) for the following reaction, H*(aq) +OH (aq)→ H2O(!) A,H° =-56.2 kJ mol-

The standard enthalpies of formation of ions in aqueous solution are obtained by arbitrarily assigning a value of zero to H* ions; that is A,H° H (aq)|=0. (a) If A,H° [HC1(g)]=-92.3 kJ mol", calculate A, H[CI (ag)] for the following reaction, HCI(g) → H(aq) + CI (aq) A,H° = -74.9 kJ mol (b) If A,H° [H,0(1)] =-285.8 kJ mol", calculate A,H° OH (aq) for the following reaction, H(aq) +OH (aq)→ H2O(!) A,H° =-56.2 kJ mol-

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter16: Spontaneity, Entropy, And Free Energy

Section: Chapter Questions

Problem 104CP: The standard enthalpy of formation of H2O(l) at 298 K is 285.8 kJ/mol. Calculate the change in...

See similar textbooks

Similar questions

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.
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.
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?
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.
Calculate the standard Gibbs free-energy change when SO3 forms from SO2 and O2 at 298 K. Why is sulfur trioxide an important substance to study? (Hint: What happens when it combines with water?)
Determine the standard Gibbs free energy change, rG, for the reactions of liquid methanol, of CO(g), and ofethyne, C2H2(g), with oxygen gas to form gaseous carbondioxide and (if hydrogen is present) liquid water at298 K. Use your calculations to decide which of thesesubstances are kinetically stable and which are thermodynamically stable: CH3OH(), CO(g), C2H9(g), CO2(g),H2O().
For the reaction BaCO3(s) BaO(s) + CO2(g), rG = +219.7 kJ/mol-rxn. Using this value and other data available in Appendix L, calculate the value of fG for BaCO3(s).
A 220-ft3 sample of gas at standard temperature and pressure is compressed into a cylinder, where it exerts pressure of 2000 psi. Calculate the work (in J) performed when this gas expands isothermally against an opposing pressure of 1.0 atm. (The amount of work that can be done is equivalent to the destructive force of about 1/4 lb of dynamite, giving you an idea of how potentially destructive compressed gas cylinders can be if improperly handled!)
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?
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.
For a process, w = 34 J and q = 109 J. What is E for this process?
Billions of pounds of acetic acid are made each year, much of it by the reaction of methanol with carbon monoxide. (AssumeT= 298 K.) CH3OH() + CO(g) CH3COOH() (a) By calculating the standard Gibbs free energy change, rG, for this reaction, show that it is product-favored. (b) Determine the standard Gibbs free energy change, rG,for the reaction of acetic acid with oxygen to form gaseous carbon dioxide and liquid water. (c) Based on this result, is acetic acid thermodynamicallystable compared with CO2(g) and H2O()? (d) Is acetic acid kinetically stable compared with CO2(g)and H2O()?