(a) What is the standard enthalpy of reaction for the reaction of 1.00 mol of propene with 1.00 mol of hydrogen to yield 1.00 mol of propane. (All gas phase) (b) What is the standard entropy change for the reaction? (c) What is the standard free energy change for the reaction carried out at 400 K? (You cannot use ∆Gfo data from the appendix). (d) Is the reaction spontaneous? (a) (b) (c) (d)

(a) What is the standard enthalpy of reaction for the reaction of 1.00 mol of propene with 1.00 mol of hydrogen to yield 1.00 mol of propane. (All gas phase) (b) What is the standard entropy change for the reaction? (c) What is the standard free energy change for the reaction carried out at 400 K? (You cannot use ∆Gfo data from the appendix). (d) Is the reaction spontaneous? (a) (b) (c) (d)

Chemistry by OpenStax (2015-05-04)

1st Edition

ISBN:9781938168390

Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Publisher:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Chapter18: Representative Metals, Metalloids, And Nonmetals

Section: Chapter Questions

Problem 41E: From the data given in Appendix I, determine the standard enthalpy change and the standard free...

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From the data given in Appendix I, determine the standard enthalpy change and the standard free energy change for each of the following reactions: (a) BF3(g)+3H2O(l)B(OH)3(s)+3HF(g) (b) BCl3(g)+3H2O(l)B(OH)3+3HCl(g) (c) B2H6(g)+6H2O(l)2B(OH)3(s)+6H2(g)
2. An experiment was carried out to determine the enthalpy change of combustion of propan-1-ol. The experimental set-up was shown below. a beaker water (500.0 cm³) propan-1-ol (a) Write the equation for the complete combustion of propan-1-ol (C;H¬OH). (b) Give a suggestion to the above set-up so as to minimize heat loss to the surroundings. (c) Burning 2.88 g of propan-1-ol caused the temperature of 500.0 cm³ of water to rise by 46.0°C. Calculate the enthalpy change of combustion of propan-1-ol. (Assume that the specific heat capacity and the density of water are 4.2 J g- K-l and 1.0 g cm- respectively.) (Molar mass of propan-1-ol: 60 g) -3 (d) The enthalpy change obtained in (c) cannot be called as 'standard enthalpy change'. Explain why.
A.) What is the heat of reaction, ΔH°? CO2(g) + H2O(l) à H2CO3(aq) –20.2 kJ mol–1 –1379 kJ mol–1 –592 kJ mol–1 B.) What is the average bond energy in CO2? CO2(g) ΔH°f, = –393.5 kJ mol–1 CO(g) ΔH°f, = –110.5 kJ mol–1 C(g) ΔH°f, = +715 kJ mol–1 CO32–(aq) ΔH°f, = –676.3 kJ mol–1 O(g) ΔH°f, = +249.0 kJ mol–1 207 kJ mol–1 1607 kJ mol–1 804 kJ mol–1
A.) Given the standard enthalpy changes for the following two reactions: (1) 2Ni(s) + O2(g)-2NIO(s) AH° = -479.4 kJ (2) Ni(s) - Cl2(g)–→NIC2(s) AH° = -305.3 kJ what is the standard enthalpy change for the reaction: (3) 2NICI,(s) + O2(g)2NIO(s) + 2C2(g) AH° = ? kJ B.) Given the standard enthalpy changes for the following two reactions: (1) 4C(s) - SH2(g) C,H10(e) AH° = -125.ó kJ (2) C,H(g)2C(s) + 2H2(g) AH° = -52.3 kJ what is the standard enthalpy change for the reaction: (3) 2C,H4(g) + H2(g) ) C,H10(g) AH° = ? kJ
Given : (a) BCl3(g) + 3H2O(l) →H3BO3(s) + 3HCl(g) ΔH = -112.5 kJ (b) B2H6(g) + 6H2O(l) →2H3BO3(s) + 6H2(g) ΔH = -493.4 kJ (c) 1/2H2(g) + 1/2Cl2(g) →HCl(g) ΔH = -92.3 kJ Calculate the value of ΔH for the reaction: B2H6(g) + 6Cl2(g) →2BCl3(g) + 6HCl(g) ΔH = ? Select one: a.-1476KJ b.-1376KJ c. -1576KJ d.-1576KJ
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Water gas, a mixture of H2 and CO, is an important industrial fuel produced by the reaction of steam with red hot coke, essentially pure carbon: C(s) + H2 O(g) ⟶ CO(g) + H2(g). (a) Assuming that coke has the same enthalpy of formation as graphite, calculate ΔH° for this reaction. (b) Methanol, a liquid fuel that could possibly replace gasoline, can be prepared from water gas and additional hydrogen at high temperature and pressure in the presence of a suitable catalyst: 2H2(g) + CO(g) ⟶ CH3 OH(g). Under the conditions of the reaction, methanol forms as a gas. Calculate ΔH° for this reaction and for the condensation of gaseous methanol to liquid methanol. (c) Calculate the heat of combustion of 1 mole of liquid methanol to H2O(g) and CO2(g).
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