Oxidation of zinc Data: Standard molar enthalpy of formation of ZnCl2 (s): A¢H°1= - 416.12 kJ mol Standard 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 HCI (g): A¡H°4 = - 72.90 kJ mol-l 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. This reaction 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 solution A,H°(Zn²*, aq).

Oxidation of zinc Data: Standard molar enthalpy of formation of ZnCl2 (s): A¢H°1= - 416.12 kJ mol Standard 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 HCI (g): A¡H°4 = - 72.90 kJ mol-l 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. This reaction 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 solution A,H°(Zn²*, aq).

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Calculate the standard enthalpy for the reaction 1/2N2(g) + 1/2O2(g) -> NO (g) given the following information: As part of your answer, show how the equations can be added together to give the overall or net equation. N2(g) + 3H2(g) -> 2NH3 (g) enthalpy = -91.8 kJ 4NH3(g) + 5O2(g) -> 4NO(g) + 6H2O(g) enthalpy= -906.2kJ H2(g) + 1/2O2 g) -> H2O(g) enthalpy+ - 241.8kJ
For the reaction 2N₂(g) + O2(g) → 2N₂O(g) AG = 214 kJ and AS = -148.5 J/K at 334 K and 1 atm. This reaction is product favored under standard conditions at 334 K. The standard enthalpy change for the reaction of 1.51 moles of N₂ (9) at this temperature would be For the reaction 2H₂O(1)→ 2H₂(g) + O₂(g) AG=483 kJ and AH = 572 kJ at 273 K and 1 atm. This reaction is reactant favored under standard conditions at 273 K. The entropy change for the reaction of 2.18 moles of H₂O(1) at this temperature would be kl. J/K.
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The enthalpy of the following reaction at 1.00 atm and 298.15K is -56.9kJmol-1 H* (ag) + OH (ag) →H,Oµ, When 2mol of an aqueous acid (H* (aq) reacts with 2mol of an aqueous base (OH(a9) in a thermally isolated constant pressure calorimeter initially at 298.15K, the temperature was observed to increase to 304.35K. In the exact same calorimeter, the hydrolysis of 1.7mol of aqueous adenosine 5'- triphosphate (ATP) caused an increase in temperature from 298.15K to 300.95K. (a) What is the enthalpy of hydrolysis per mol of ATP? (b) The hydrolysis of ATP is the primary mechanism by which the energy required by the human body is released. Assuming that the human body can use all of the released energy from ATP hydrolysis, how many grams of ATP is necessary to undergo hydrolysis per day to provide the average human daily energy requirement of 2000kcals (Molar mass of ATP =507.181gmol-1), assuming no other source of energy.
The hydrocarbons acetylene (C2H2) and benzene (C6H6)have the same empirical formula. Benzene is an “aromatic”hydrocarbon, one that is unusually stable because of its structure.(a) By using data in Appendix C, determine the standardenthalpy change for the reaction 3 C2H2(g)-----> C6H6(l).(b) Which has greater enthalpy, 3 mol of acetylene gas or1 mol of liquid benzene? (c) Determine the fuel value, inkJ/g, for acetylene and benzene.
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