2 NO (g) + O2 (g) --> 2 NO2 (g) Without doing any calculations, predict the sign

Question

2 NO (g) + O2 (g) --> 2 NO2 (g)
Without doing any calculations, predict the sign of delta S°rxn and delta H °rxn, and explain your predictions. (Hint: what is the sign of delta G°? Can you use this information to figure out the other two?) 2 NO (g) + O2 (g) --> 2 NO2 (g)
Without doing any calculations, predict the sign of delta S°rxn and delta H °rxn, and explain your predictions. (Hint: what is the sign of delta G°? Can you use this information to figure out the other two?) 1. (3 pts) The following process is spontaneous at 25 °C e following process 1S 2 NO (g) + O2 (g) 2 NO2 (g) without doing any calculations, predict the sign ofAS , and AHP and explain your predictions. (Hint-what is the sign of Gm Can you use this information to figure out the other two?)

Explanation / Answer

The following processes spontaneous at 25°C:

2 NO (g) + O2 (g) --> 2 NO2 (g)

Without doing any calculations, predict the sign of delta S°rxn and delta H°rxn, and explain your predictions. (Hint: what is the sign of delta G°? Can you use this information to figure out the other two?)

delta S^0 rxn for this reaction is negative because reactant side has 4 moles of gases where as product side has only 2

In spontaneous reactions the entropy is increases and enthalpy decrease.

All spontaneous reactions have a negative free-energy change, if free-energy change is positive than the reaction is non-spontaneous.

Thus the sign of delta S is negative and the sign of delta H is positive.

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