Consider the spontaneous combustion reaction of hydrogen and oxygen to form wate
ID: 586890 • Letter: C
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 UpExplanation / Answer
1) delta S system is negative ,as the degree of randomness decreases in the liquid than in the gas . 2) no , Gibbs free energy determines the spontaneity 3)as delta h is negative reaction is exothermic 4)as the reaction is exothermic ,the temperature of surrounding increases.