A liquid compound freezes into solid state, which is accompanied by 58.8 kJ of heat transferred to the surroundings at a constant pressure and a constant temperature of 301.1 K. What is the entropy change of surroundings (ASsurroundings) in unit of J/K for this process? Please keep your answer to one decimal place. A Moving to another question will save this response. « K Question 8 of 11>»

Consider the two different systems, A and B, shown below.  If there are 3 particles with a total energy of 12 J, which system would have more entropy and why? Question 21 options:   System A has more entropy because it has greater separation between energy levels and hence more microstates than system B.   System B has more entropy because it has more than two microstates, whereas System A only has two microstates possible.   System A has more entropy because it has three microstates, whereas System B has less than three microstates possible.   System B has more entropy because it has more than three microstates, whereas System A only has three microstates possible.   System A has more entropy because it has more than one microstate, whereas System B only has one microstate possible.

8 As you dissolve salt in water, what change would you expect to occur? A B C D The entropy of the system will increase. The kinetic energy of the water molecules decreases. The salt consumes energy as it transfers entropy The water molecules become more closely packed as the temperature increases

Read the descriptions of physical or chemical changes in the table below. Then decide whether the change will be spontaneous, if you can. Change A gas condenses to a liquid, neither absorbing nor releasing heat. An exothermic chemical reaction between a solid and a liquid results in gaseous products. Two liquids mix, neither absorbing nor releasing heat. Is this change spontaneous? Yes. No. Can't decide with information given. ○ Yes. ○ No. Can't decide with information given. Yes. No. ○ Can't decide with information given.

What is the entropy change, in J mol-1 K-1, when 100.0 g of water boils at 100.0 oC?  (ΔHvaporization = 40.7 kJ/mol)  Type in your answer as a whole number with no units.

Compare what will happen to the entropy of the whole system in the following two scenarios: A) if the oil molecules are all clumped together and the clump is surrounded by water and B) if the oil molecules are spread out evenly throughout the water, each individual oil molecule surrounded by water?

Evaluate each reaction below and using your knowledge of entropy, predict whether entropy will increase or decrease as reactants are converted to products. Reaction Will entropy increase or decrease? 2 NH3(g) → N2(g) + 3 H2(g)      increase or decrease PbS(s) → Pb2+(aq) + S2-(aq)  increase or decrease  CH4(g) + 2 O2(g) → CO2(g) + 2 H2O(l)  increase or decrease N2(g) + 3 H2 (g) → 2 NH3 (g)  increase or decrease

25. H2(g) + I2(g) 2HI(gx Kp = 55.2 AH°rxn = +53 kJ Write the formulas for Kp and Qp of this equation: Kp = Qp = A mixture with 0.22 atm H2(g), 0.05 atm I2(g), and 3.5 atm HI(g) has Qp = and will shift to: (show direction) to reach equilibrium. If the mixture at equilibrium is heated, it will shift to: to reach new equilibrium.