It follows that the reaction is spontaneous at high temperatures Option A.
<h3>What is ΔS ?</h3>
The term ΔS is referred to as the change in the entropy of the system. Now recall that entropy is defined as the degree of disorderliness in a system. If a system is highly disorderly then it means that it has a high entropy. Also, ΔH has to do with the heat change that accompanies a reaction.
We know that both the entropy and the heat change can both either be positive or negative. Now we know that the equation ΔG = ΔH - TΔS can be used to ascertain whether or not a reaction will be spontaneous. If the result is negative, then the reaction will be spontaneous.
As such, when then it follows that the reaction is spontaneous at high temperatures Option A.
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Answer:
Their vibrations speed up
Explanation:
They start vibrating faster and faster and start generating more and more heat and separate from each other so, therefore (usually), become less dense
Answer:
310.69K
Explanation:
Given parameters:
Initial temperature T₁ = 292K
Initial pressure P₁ = 1.25atm
Final pressure P₂ = 1.33atm
Unknown:
Final temperature T₂ = ?
Solution
To find the unkown, we need to apply the combined gas law. From the combined gas law, it can be deduced that at constant volume, the pressure of a give mass or mole of gas varies directly with the absolute temperature.
Since the same aerosol can is heated, the volume is constant.
= 
Now, we have to make T₂ the subject of the formula:
T₂ = 
T₂ = 
= 310.69K
