Many air fresheners are in solid form at normal atmospheric pressure and room temperature. However, they undergoes sublimation (changes from solid to gas phase) when heated to release fragrant scents, such as when they are plugged into an electrical outlet. According to the second law of thermodynamics, what must be true about entropy changes in this example? Select the correct answer below: AS sys +AS surr 0 ASsys + ASsurr< 0 ASsys+ASsurr >0 Insufficient information is provided to determine the direction of entropy change.

Classify each statement as true or false. Statement True or false? For any spontaneous process, the ΔSsys must be positive.     For the reaction Mg(s) + Cl2(g) → MgCl2(s), the sign of ΔSsys is positive.     Increasing the temperature of a system increases the number of microstates.

A hot rock ejected from a volcano’s lava fountain cools from 1100C to 40.0C, and its entropy decreases by 950 J/K. How much heat transfer occurs from the rock?

Calculate the change of the entropy of the system in J/K for the following phase transition: condensation of 64.1 g methanol The molar mass of methanol (CH3OH) is 32.04 g/mo%; the enthalpy of vaporization of methanol is 37.6 kJ/mol; the boiling point of methanol is 64.7°C A) -3640 B) -1130 C) 1.13446677 D) -223 E) 0.22258

Consider the combustion of propane gas:  C3H8(g)    +     5O2(g)           ------>           3CO2(g)        +            4H2O(g)            ΔHrxn  =  - 2044 kJ  Determine the sign of the entropy change for the system.

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.

. Chloroform, CHC13, has a normal boiling point of 61 °C and it enthalpy of vaporization is 29.24 kJ/mol, what is its entropy of vaporization in J/mol·K at 61 °C? Before you calculate it write a chemical equation for this process and predict do you expect entropy to be positive or negative?

Nitric oxides, NONO and NO2NO2, contribute to air pollution, acid rain, and the depletion of the ozone layer. After NONO forms in the combustion chamber of an automobile engine, it reacts further with oxygen to form NO2NO2. The reaction is given by: 2NO(g)+O2(g)→2NO2(g). Calculate ΔS∘rxn for the reaction?   Entropy values given by following table SubstanceSubstance S∘ (J/mol⋅K)S∘ (J/mol⋅K) NO2NO2 240.0 O2O2 205.2 NONO 210.8

Calculate the entropy (in J/K) change when 866.7 g of liquid cyclohexane, C6H12, freezes at 6.47°C. The boiling point is 80.74°C, the melting point is 6.47°C, the enthalpy of vaporization is 32.0 kJ/mol, and the enthalpy of fusion is 2.68 kJ/mol for cyclohexane. Report your answer to 3 sig figs, but do NOT include units.

The normal boiling point of ethanol, C2H5OH, is 78.3°C, and its molar enthalpy of vaporization is 38.56KJ/mol. What is the change in entropy in the system when 68.3 g of ethanol vapor at 1 atm condenses to liquid at the normal boiling point? O 163J/K O 160J/K O -163 J/K O -160J/K