(a) How much does the free energy (kJ/mole) of 15 g of pure Cu change by adding 5 g of pure Zn at a temperature of 1100 degrees C? Assume an ideal solution, and that Go(Cu) = -1200 kJ/mole, and Go(Zn) = -2000 kJ/mole at this temperature. A(Cu) = 63.55, and A(Zn) = 65.39. b) By how much more does the system free energy change by adding 5 g of Ga to the mixture in part a)? A(Ga) = 69.7, and Go(Ga) = - 3000 kJ/mole. %3D %3D

(a) How much does the free energy (kJ/mole) of 15 g of pure Cu change by adding 5 g of pure Zn at a temperature of 1100 degrees C? Assume an ideal solution, and that Go(Cu) = -1200 kJ/mole, and Go(Zn) = -2000 kJ/mole at this temperature. A(Cu) = 63.55, and A(Zn) = 65.39. b) By how much more does the system free energy change by adding 5 g of Ga to the mixture in part a)? A(Ga) = 69.7, and Go(Ga) = - 3000 kJ/mole. %3D %3D

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...

See similar textbooks

Similar questions

Given the standard enthalpy changes for the following two reactions:(1) 2Fe(s) + O2(g) -> 2FeO(s)...... ΔH° = -544.0 kJ(2) 2Zn(s) + O2(g) -> 2ZnO(s)......ΔH° = -696.6 kJwhat is the standard enthalpy change for the reaction:(3) FeO(s) + Zn(s) -> Fe(s) + ZnO(s)......ΔH° = ?_____ kJ
Now consider the following set of reactions: 1. CO + O₂ CO₂, AH= -283 kJ/mol 2. CO₂ CO₂, AH=-393 kJ/mol
Calculate the standard enthalpy of reaction for: C2H2 ---> 2 C + H2 If, 2 C2H2 + 5 O2 ----> 4 CO2 + 2 H2O (Standard Enthalpy = -2600 kJ/mole) C + O2 ---> CO2 (Standard Enthalpy = -390 kJ/mole) 2 H2 + O2 ---> 2 H2O (Standard Enthalpy = -590 kJ/mole)
Question 15.62
The burning of 48.7 g of ZnS in the presence of oxygen gives 220.0 kJ of heat. What is ΔH for the reaction as written below? 2 ZnS + 3 O2 ----> 2 ZnO + 2 SO2 a) -110 kJ b) -293 kJ c) -441 kJ d) -882 kJ e) +441 kJ
1. How much energy in kJ is released when 124.49 g of nickel react with an excess of phosphorus? 5 Ni + 2 P -> Ni5P2 △ H = 436 kJ/mol 2.How much titanium in grams is required to release 538.13 kJ of heat? Ti + 2 B -> TiB2 △ H = 316 kJ/mol
Q3/ from the following reaction 4FEO + O2 2FE2O3 -570 kJ/mole 1- Calculate the heat of reaction per mole FeO 2- If 3600 mole of Fe2O3 produced from this reaction, calculate the total heat (produced or absorbed) 3 – If the reaction formula changed to the following formula, calculate the heat of reaction 8FEO + 2 O2 4FE2O3
Using the provided enthalpy of formation, determine the enthalpy for the reaction: 3A (s)+ 2B (I) ->C (I) + 4D(s) substance AH;° (KJ/mol) A (s) -286
Under certain nonstandard conditions, oxidation by O2( g) of1 mol of SO2( g) to SO3( g) absorbs 89.5 kJ. The enthalpy of formationof SO3( g) is -204.2 kJ under these conditions. Find theenthalpy of formation of SO2( g).
Given that: AH°F [Fe(OH)3 (s) ] =- 823.0 kJ/mol AH°f [Fe+3 (aq)] = - 48.5 kJ/mol AH°F [OH (aq)] = - 230.0 kJ/mol What is the enthalpy change for the precipitation reaction of Fe(OH)3 (s)? O A.-344.5 kJ/mol O B.-1101.5 kJ/mol Oc-1561.5 kJ/mol -447.5 kJ/mol O D. O E. :- 84.5 kJ/mol
Using the equation for photosynthesis below, answer the following equations 2800kJ + 6 CO: (g) + 6 HeO () > CeHi2Oe (s) + 6 02 (g)
Calculate ΔH° in kilojoules for the following reaction, the preparation of the unstable nitrous acid, HNO2. Use the following thermochemical equations: