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    without doing any calculations, determine the sign of δssys for each of the following chemical reactions.

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    Without doing any calculations, determine the sign of ΔSsys and ΔSsurr for each of the chemical reaction. Predict under what temperatures (all, low, or high), if any, the reaction will be spontaneous? C3H8(g)+5O2(g)→3CO2(g)+4H2O(g) ΔH_"rxn"^o =−2044kJ

    DeltaS_{sys}>0 DeltaS_{surr}>0 DeltaS_{uni}>0 All temperature will be spontaneous. DeltaS_{sys}>0 as there are more gaseous products than reactants. DeltaS_{surr}>0 as heat is released to the surroundings. DeltaS_{uni}>0 as both DeltaS_{sys} and DeltaS_{surr}>0 are negative. At all temperature, the above hold true. DeltaS_{uni}>0 implies that the reaction will be spontaneous at all temperatures.

    Without doing any calculations, determine the sign of ΔSsys and ΔSsurr for each of the chemical reaction. Predict under what temperatures (all, low, or high), if any, the reaction will be spontaneous? C3H8(g)+5O2(g)→3CO2(g)+4H2O(g)

    Δ H o rxn = − 2044 k J

    Chemistry Thermochemistry Entropy

    1 Answer

    Bio Nov 3, 2015 Δ S s y s > 0 Δ S s u r r > 0 Δ S u n i > 0

    All temperature will be spontaneous.

    Explanation:

    Δ S s y s > 0

    as there are more gaseous products than reactants.

    Δ S s u r r > 0

    as heat is released to the surroundings.

    Δ S u n i > 0 as both Δ S s y s and Δ S s u r r > 0 are negative.

    At all temperature, the above hold true.

    Δ S u n i > 0

    implies that the reaction will be spontaneous at all temperatures.

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    Without doing any calculations, determine the sign of ΔSsys for e...

    Without doing any calculations, determine the sign of ΔSsys for each chemical reaction. a. 2 KClO3(s) ¡ 2 KCl(s) + 3 O2( g)

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    Without doing any calculations, determine the sign of ΔSsys for each chemical reaction. a. 2 KClO3(s) ¡ 2 KCl(s) + 3 O2( g)

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