Determine whether entropy increases or decreases for the processes shown below. Entropy increases No Answers Chosen Entropy does not change !!!! No Answers Chosen Possible answers 2 N2O(g) -> 2 N2(g) + O2(g) Solid CO2 sublimes CaCO3(s)-> CaO(s) + CO2(g) Entropy decreases No Answers Chosen Water vapour condenses 2 H2S(g) + 3 O2(g) -> 2 H2O(g) +2 SO2(g) Mg(s) + C12(g) -> MgCl2(s)

1.  Ammonia can be made from the reaction of nitrogen and hydrogen: N2  (g)  +  3 H2 (g)      ⟺        2 NH3 (g) For this reaction, K = 1.6 x 102 and ΔH = -91.8 kcal/mole at 25oC. Is the reaction endothermic or exothermic? Briefly explain. Is there in increase in entropy, a decrease in entropy, or no change in entropy?  Briefly explain. At 25oC, is this reaction product favored or reactant favored? Briefly explain. Do you expect this reaction to be spontaneous at all temperatures?  Briefly explain.

For each system listed in the first column of the table below, decide (if possible) whether the change described in the second column will increase the entropy  S  of the system, decrease  S , or leave  S  unchanged. If you don't have enough information to decide, check the "not enough information" button in the last column. System Change S A few moles of carbon dioxide (CO2) gas. The carbon dioxide is heated from 9.0 °C to 36.0 °C and also expands from a volume of 6.0 L to a volume of 14.0 L.     <S0     =S0     >S0     not enough information A few moles of helium (He) gas. The helium expands from a volume of 9.0 L to a volume of 15.0 L while the temperature is held constant at 20.0 °C.     <S0     =S0     >S0     not enough information A few grams of liquid ammonia (NH3). The ammonia is heated from -1.0 °C to 2.0 °C.     <S0…

1:44 1 LTE 4 1 Search Question 20.b of 23 Show Answer Consider the reaction Cl2(g) + Br2(g) → 2 BrCI(g) at 25 °C. Which of the following best explains why the change in entropy is so small? A) All of the components in the chemical equation are gases. B) There are the same moles of gas on both sides of the reaction. C) The temperature of the reaction does not change. Tap here or pull up for additional resources