Consider the reaction between nitrogen and oxygen gas to form nitrogen dioxide:

Question

Consider the reaction between nitrogen and oxygen gas to form nitrogen dioxide:
N2(g)+2O2(g)2NO2(g)Hrxn=+66.4kJ

Part A

Calculate the entropy change in the surroundings associated with this reaction occurring at 25 C.

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Part B

Determine the sign of the entropy change for the system.

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Part C

Determine the sign of the entropy change for the universe.

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Part D

Is the reaction spontaneous?

Consider the reaction between nitrogen and oxygen gas to form nitrogen dioxide:
N2(g)+2O2(g)2NO2(g)Hrxn=+66.4kJ

Part A

Calculate the entropy change in the surroundings associated with this reaction occurring at 25 C.

Ssurr=

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Part B

Determine the sign of the entropy change for the system.

Determine the sign of the entropy change for the system. negative positive

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Part C

Determine the sign of the entropy change for the universe.

Determine the sign of the entropy change for the universe. negative positive

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Part D

Is the reaction spontaneous?

Is the reaction spontaneous? yes no

Explanation / Answer

Part (A)

Delta (S) = - Delta (H) / T

Delta (S) = 66400 J / ( 273 +25) = 222.81 J / K

Part (B)

Delta (S) will be negative ( 3 moles of gas on reactant side and 2 moles of gas on product side)

Part (C)

Delta (S) = Delta (S) + Delta (S) = since the entropy change of both system and surrounding are negative so will the entropy change of universe.

Part (D)

The reaction will not occur spontaneously.

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