Answer:
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Explanation:
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The answer is true. According to the second law of thermodynamics, energy tends to become more spread out
Answer:
Lowering the temperature typically reduces the significance of the decrease in entropy. That makes the Gibbs Free energy of the reaction more negative. As a result, the reaction becomes more favorable overall.
Explanation:
In an addition reaction there's a decrease in the number of particles. Consider the hydrogenation of ethene as an example.
.
When
is added to
(ethene) under heat and with the presence of a catalyst,
(ethane) would be produced.
Note that on the left-hand side of the equation, there are two gaseous molecules. However, on the right-hand side there's only one gaseous molecule. That's a significant decrease in entropy. In other words,
.
The equation for the change in Gibbs Free Energy for a particular reaction is:
.
For a particular reaction, the more negative
is, the more spontaneous ("favorable") the reaction would be.
Since typically
for addition reactions, the "entropy term" of it would be positive. That's not very helpful if the reaction needs to be favorable.
(absolute temperature) is always nonnegative. However, lowering the temperature could help bring the value of
Scientists make hypothesis in order to make an educated guess on the outcome of the experiment.