Oxidation of zincData:Standard molar enthalpy of formation of ZnCl2 (s): A¡H°1 = - 416.12 kJ mol-lStandard molar enthalpy of formation of HCl (g): A¢H°2 = - 92.08 kJ mol·'Standard molar enthalpy of dissolution of ZnCl2 (s): A;H°3= - 65.71 kJ mol-'Standard molar enthalpy of dissolution of HCl (g): A;H°4 = - 72.90 kJ mol-'Standard molar enthalpy of formation of H† (aq): A;H°(H†, aq) = 0 kJ mol·'Let's consider the reaction of oxidation of zinc by the solvated proton in the aqueous phase. Thisreaction is represented by the chemical reaction (1):(1) Zn (s) + 2H+ (aq) → Zn²+ (aq) + H2 (g)Calculate the standard molar enthalpy for reaction (1).. Calculate the standard molar enthalpy of formation of the zinc cation Zn2* in aqueous solutionA;H°(Zn²*, aq).

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Answered: Oxidation of zinc Data: Standard molar…

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter12: Thermodynamic Processes And Thermochemistry

Section: Chapter Questions

Problem 84AP

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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?
The distance between downtown San Francisco and downtown Oakland is 9 miles. However, a car driving between the two points travels 12.3miles. Of these distances, which one is analogous to a state function? Why?
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.
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?
Dissolving 6.00 g CaCl2 in 300 mL of water causes the temperature of the solution to increase by 3.43 C. Assume that the specific heat of the solution is 4.18 J/g K and its mass is 306 g. (a) Calculate the enthalpy change when the CaCl2 dissolves. Is the process exothermic or endothermic? (b) Determine H on a molar basis for CaCl2(s)H2OCa2+(aq)+2Cl(aq)
Given the following standard enthalpies of hydration; Mg 2 + (g) + (ag) Mg2+(aq); A110 - 1920KJ C-n (g) + (aq) CT (a q) ; All 0 - 364 KJ- and using the value of AHO for the reaction a!ready given; calculate the standard enthalpy of solution of magnesium chloride.
The standard heat of formation for Ag2CrO4(s) is -712 kJ/mol at 298 K. Write the formation equation for Ag2CrO4(s) that goes with this value of ΔH
When ethanol burns in oxygen under standard conditions, carbon dioxide, water and 1368 kJmol-1 of energy are produced. Calculate the enthalpy of formation of ethanol, given that the enthalpies of formation of carbon dioxide and water are -393.7 and -285.9 kJmol-1 respectively.
A student poured 100 ml of water (density = 1.00 g / mL) into a coffee calorimeter, noted that the temperature of the water was 18.8oC, then added 5.33 g KOH. With the lid on, the mixture was stirred, temperature increased and the maximum temperature reached at the time of mixing 31.6 oC. Calculate the heat of the system in this dissolution reaction (qsys). ( Approximate the specific heat capacity, cp as 4.18 J g-1 K-1. Do not consider the contribution to the heat generated from the calorimeter; assume that this is zero. Only calculate the heat from the heat capacity of the solution. make sure you consider the sign of qsys qsys for dissolution of KOH = J
Titanium can be produced by electrolytic reduction from an anhydrous molten salt electrolyte that contains titanium(IV) chloride and a spectator salt that furnishes ions to make the electrolyte conduct electricity. The stan- dard enthalpy of formation of TiCl4(liquid) is -750 kJ mol^-1, and the standard entropies of TiCl4(liquid), Ti(s), and Cl2(g) are 253, 30, and 223 J K^-1 mol^-1, respectively. What minimum applied voltage will be necessary at 100°C?

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