We’re being asked to predict which has the greatest entropy (ΔS) for the given reactions. Recall that if:
• ΔS > 0 or ΔS = (+); entropy is increased
• ΔS < 0 or ΔS = (–); entropy is decreased
Remember that phase changes lead to a change in entropy:
For each pair of substances, at the same temperature, choose the one with the higher entropy:
I. (i) I2(l) (ii) I2(s)
II. (i) PCl3(g) (ii) PCl5(g)
III. (i) BaI2(aq) (ii) BaI2(s)
IV. (i) 2 moles of NO2(g) (ii) 1 mole of N2O4(g)
a. (ii) (i) (i) (i)
b. (i) (ii) (i) (ii)
c. (i) (i) (ii) (i)
d. (ii) (ii) (i) (i)
e. (i) (ii) (i) (i)
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What scientific concept do you need to know in order to solve this problem?
Our tutors have indicated that to solve this problem you will need to apply the Entropy concept. You can view video lessons to learn Entropy. Or if you need more Entropy practice, you can also practice Entropy practice problems.
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Based on our data, we think this problem is relevant for Professor Goodwin's class at HCC.