For the reaction NO ( g ) + NO 2 ( g ) → N 2 O 3 ( g ) , use tabulated thermodynamic data to calculate Δ H ° and Δ S ° . Then use those values to answer the following questions. (a) Is this reaction spontaneous at 25°C? Explain your answer. (b) If the reaction is not spontaneous at 25°C, will it become spontaneous at higher temperatures or lower temperatures? (c) To show that your prediction is accurate, choose a temperature that corresponds to your prediction in part (b) and calculate Δ G . (Assume that both enthalpy and entropy are independent of temperature.)
For the reaction NO ( g ) + NO 2 ( g ) → N 2 O 3 ( g ) , use tabulated thermodynamic data to calculate Δ H ° and Δ S ° . Then use those values to answer the following questions. (a) Is this reaction spontaneous at 25°C? Explain your answer. (b) If the reaction is not spontaneous at 25°C, will it become spontaneous at higher temperatures or lower temperatures? (c) To show that your prediction is accurate, choose a temperature that corresponds to your prediction in part (b) and calculate Δ G . (Assume that both enthalpy and entropy are independent of temperature.)
Solution Summary: The author explains how to calculate the entropy changes, define spontaneity of reaction, and temperature dependence.
For the reaction
NO
(
g
)
+
NO
2
(
g
)
→
N
2
O
3
(
g
)
, use tabulated thermodynamic data to calculate
Δ
H
°
and
Δ
S
°
. Then use those values to answer the following questions.
(a) Is this reaction spontaneous at 25°C? Explain your answer.
(b) If the reaction is not spontaneous at 25°C, will it become spontaneous at higher temperatures or lower temperatures?
(c) To show that your prediction is accurate, choose a temperature that corresponds to your prediction in part (b) and calculate
Δ
G
. (Assume that both enthalpy and entropy are independent of temperature.)
Science that deals with the amount of energy transferred from one equilibrium state to another equilibrium state.
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The Laws of Thermodynamics, Entropy, and Gibbs Free Energy; Author: Professor Dave Explains;https://www.youtube.com/watch?v=8N1BxHgsoOw;License: Standard YouTube License, CC-BY