Consider the spontaneous combustion reaction of hydrogen and oxygen to form wate

Question

Consider the spontaneous combustion reaction of hydrogen and oxygen to form water 2H2(g) + O2(g)2H3O(1) Hsystern =-483kJ Part B-Predicting the entropy change for the system. 5,ystem, from the balanced equation Positive Predicting the entropy change for the system, ASsystem, from the balanced equation Negative Is ASsystem positive or negative? Is this entropy change a driving force for spontaneity? Yes No Predicting how the enthalpy change for the system, ,ystem, affects assum Based on the sign of AHsystem, is this reaction endothermic or exothermic? Does the temperature of the surroundings increase or decrease? Is ASsurroundings positive or negative? Is this enthalpy change a driving force for spontaneity? Endothermic Exothermic Increase Decrease Consider the signs of AS you determined above and that ASuniverse ASsystem +ASsurroundings syatem Given that this reaction is spontaneous at 298K, which value should be larger in magnitude at 298K, ASsystem or ASsurroundings? AS Reset Help Submit My Answers Give Up

Explanation / Answer

Q1

a)

dSsystem must be negative, since 2+1 = 3 mol of gas forms 2 mol fo liquid

entropy of liquid << entropy of gas

b)

entropy is NOT the driving force for spontaneos process

Q2

since dH system is negative, ti is exothermic, it releases heat

T must increase, since heat is being released

dSsurr = depends on heat, so it must be increasing due to exothermic reaction

dH = drives spotnaneous (YES)

Q3

dSuniverwse must be possible, given that dH <<< dS

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