Consider a reaction that has a positive delta H and a positive delta S. Which of

Question

Consider a reaction that has a positive delta H and a positive delta S. Which of the following statements is TRUE? A) This reaction will be nonspontaneous at all temperatures. B) This reaction will be spontaneous at all temperatures. C) This reaction will be spontaneous only at low temperatures. D) This reaction will be non spontaneous only at low temperatures. E) It is not possible to determine without more information. For the following example, identify the following. 3O_2(g) rightarrow 2O_3(g) A) a negative delta H and a positive delta S B) a positive delta H and a negative delta S C) a negative delta H and a negative delta S D) a positive delta H and a positive delta S E) It is not possible to determine without more information. Below what temperature does the following reaction become nonspontaneous? 2 HNO_3(aq) + NO(g) rightarrow 3NO_2 (g) + H_2 O(1) delta H = +136.5 kJ: delta S = +287.5 J/K A) 151 K B) 39.2 K C) 475 K D) This reaction is nonspontaneous at all temperatures. E) This reaction is spontaneous at all temperatures. Identify the statement that is FALSE. A) Free atoms have greater entropy than molecules. B) Entropy increases with dissolution. C) For noble gases, entropy increases with size. D) The entropy of a gas is greater than the entropy of a liquid. E) Entropy generally increases with increasing molecular complexity. Which one of the following has the highest standard molar entropy, S^o, at 25 degree C? A) O_2(g) B) H_2(g) C) Cl_2(g) D) F_2(g) E) N_2(g)

Explanation / Answer

Question 1.

If dH and dS are positive

then

dG = dH - T*dS

we need dG to be negtive for this process to be spontaneous

so

we will require numerical vlaue for dH and dS

therefore

E) impossilbe without more information

Question 2.

Note that

mol of gas increases ---> increase in entropy

the reaction is endothermic, so dH = positive

both are positive

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