Q2. Consider the hydrogenation of ethyleneC2H4 + H2 = C2H6The heats of combustion and molar entropies for the three gases at 298 K are given by:C2H4C2H6H2AH comb/kJ mol¹-1395-1550-243Sº / J K¹ mol-1220.7230.4131.1The average heat capacity change, ACP, for the reaction over the temperature range 298-1000 K is10.9 J K¹ mol¹. Using these data, determine:(a) the standard enthalpy change at 800 K(b) the standard entropy change at 800 K(c) the equilibrium constant at 800 K.

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Answered: Q2. Consider the hydrogenation of…

Physical Chemistry

2nd Edition

ISBN:9781133958437

Author:Ball, David W. (david Warren), BAER, Tomas

Publisher:Ball, David W. (david Warren), BAER, Tomas

Chapter2: The First Law Of Thermodynamics

Section: Chapter Questions

Problem 2.85E: Natural gas is mostly CH4. When it burns, the chemical reaction is CH4 g 2O2 g CO2 g 2H2O g The H...

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What are the two ways that a final chemical state of a system can be more probable than its initial state?
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?
Describe why it is easier to use Gto determine the spontaneity of a process rather than S u
Calculate rS for each substance when the quantity of thermal energy indicated is transferred reversibly to the system at the temperature specified. Assume that youhave enough of each substance so that its temperatureremains constant as the thermal energy is transferred. (a) H2(g), 0.775 kJ/mol, 295 K (b) KCl(s), 500. kJ/mol, 500. K (c) N2(g), 2.45 kJ/mol, 1000. K
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.
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.
Why is it usually easier to use G to determine the spontaneity of a process rather than Su ?
You have a 1.00-L sample of hot water (90.0C) sitting open in a 25.0C room. Eventually the water cools to 25.0C while the temperature of the room remains unchanged. Calculate Ssurr for this process. Assume the density of water is 1.00 g/cm3 over this temperature range, and the heat capacity of water is constant over this temperature range and equal to 75.4 J/K mol.
The enthalpy of vaporization for water is 40.65 kJ mol-1. As a design engineer for a project in a desert climate, you are exploring the option of using evaporative cooling. (a) If the air has an average volumetric heat capacity of 0.00130 J cm-3 K-1, what is the minimum mass of water that would need to evaporate in order to cool a 5 m? 5 m room with a 3 m ceiling by 5°F using this method? (b) Is this a spontaneous or nonspontaneous process?
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!)
The octane number of gasoline is based on a comparison of the gasolines behavior with that of 2,2,4-trimethylpentane, C8H18(), which is arbitrarily assigned an octane number of 100. The standard enthalpy of combustion of this compound is 5456.6 kJ/mol. (a) Write the thermochemical equation for the combustion of 2,2,4-trimethylpentane. (b) Use the standard enthalpies of formation in Appendix G to calculate the standard enthalpy of formation of 2,2,4-trimethylpentane.
A 2.50-mol sample of gas is compressed isothermally from 20.0 L to 5.00 L under a constant external pressure of 10.0 atm. Calculate w, q, U, and H for the process.

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