Indicate which of the following has the lowest stan CH_4(g) CH_3CH_2OH(l) H_2O(s
ID: 487104 • Letter: I
Question
Indicate which of the following has the lowest stan CH_4(g) CH_3CH_2OH(l) H_2O(s) Na(s) He(g) Indicate which one of the following reactions result in a positive delta S_sys. AgNO_3(aq) + NaCl(aq) doublesidearrow AgCl(s) + NaNO_3(aq) HCl(g) + H_2O(l) doublesidearrow HCl(aq) H_2(g) + I_2(g) doublesidearrow 2HI(g) C_2H_2O_2(g) doublesidearrow 2CO(g) + H_2(g) H_2O(g) doublesidearrow H_2O(l) Determine the entropy change for the reaction, SO_2(g) + 1/2 O_2(g) rightarrow SO_3(g), given the following: -196.4 J/K +196.4 J/K -93.9 J/K +93.9 J/K +401.4 J/K Processes are always spontaneous when ___ (H and S refer to the system). delta H > 0 and delta SExplanation / Answer
Answer of (1)
Higher entropy = more random/disorganized.
Lower entropy = less random/disorganized.
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A few general rules for predicting entropy changes:
1. Gases are more random than liquids which are more random than solids.
Order of increasing entropy: (s) < (l) < (g)
If the states are the same, then an increase in number of moles would mean an increase in entropy.
So the Na is solid state as well as lesser number of mole so Na has lower standard molar entropy.
so Answer is (d) Na
Answer(2)
d. C2H2O2(g) = 2 CO(g) + H2(g)
Answer(3)
(c) –93.9 J/K
Answer(4)
(d) H < 0 and S > 0
Answer(5)
G = H - TS
= (-92.38 KJ) - {623 K x (-0.1982 KJ/mol K)}
= 31.1 KJ/mol
(e) 31.1 kJ/mol