a) Calculate the entropy change of the system, surroundings and the universe(total) for the following spontaneous reaction at 298K at constant pressure: N2(g) + 3H2(g) ====> 2NH3(g)b) Calculate the entropy change of the system for the reaction at 198K (assume the relevant heat capacities are temperature independent)

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itsmevLv7

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Patrina SchowalterLv2

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Related questions

1. For each of the following statements, indicate whether it is true or false, and briefly explain your reasoning.

a) A spontaneous reaction always releases heat.

b) A spontaneous reaction is always a fast reaction.

c) The entropy of a system always increases for a spontaneous change.

d) The entropy of a system and its surroundings always increases for a spontaneous change.

e) The energy of a system always increases for a spontaneous change.

2. The reaction shown below is spontaneous at room temperature, but becomes nonspontaneous at a much higher temperature:

N2(g) + 3H2(g) --> 2 NH3(g)

From this fact alone, determine the signs of ÎHÂ° and ÎSÂ°, assuming that these do not change much with temperature. Explain your reasoning.

blueferret259

Consider the condensationof 0.50 mol of ethanol vapor at 38.3oC and 1bar.

Calculate the heat, theentropy change for the system, the entropy change forthe surroundings and the total entropy change forthe universe. What does the sign of DRSo Universe tell you?

The boiling point ofethanol under a pressure of 1 bar is 78.3oC and at this temperatureDvapHo = 39.3kJ.mol%u20101. Thestandard molar heat capacities at constant pressure for ethanolliquid and vapor are 111.46 and 65.44 J/K.mol,respectively.

Consider the reaction between graphite and oxygen gas to form carbon monoxide:

2C (s) graphite + O2 (g) → 2CO (g) ΔH_rxn = −221.0kJ

Calculate the entropy change in the surroundings associated with this reaction occurring at 25 ^∘C.
Determine the sign of the entropy change for the system.
Determine the sign of the entropy change for the universe.
Is the reaction spontaneous?