For a process to be at equilibrium, it is necessary
that
ΔSsys = 0 and
ΔSsurr = 0.
ΔSsys = ΔSsurr.
ΔSsys = 0.
ΔSsys =
-ΔSsurr
Ans : ΔSsys = -ΔSsurr
For a process to be at equillibrium , the entropy change of the system must be equal and opposite to the entropy change of the surroundings.
The change in entropy of system and change in entropy of surroundings add to the change in entropy of the universe , which is equal to zero for an ideal reversible process.
For a process to be at equilibrium, it is necessary that ΔSsys = 0 and ΔSsurr = 0....
Without doing any calculations, determine the sign of ΔSsys and ΔSsurr for each of the chemical reactions below. Part A 2CO(g)+O2(g)⇌2CO2(g)ΔH∘rxn= -566.0 kJ -566.0 ΔSsys>0, ΔSsurr>0 ΔSsys<0, ΔSsurr>0 ΔSsys>0, ΔSsurr<0 ΔSsys<0, ΔSsurr<0 SubmitMy AnswersGive Up Part B 2NO2(g)→2NO(g)+O2(g)ΔH∘rxn= +113.1 kJ +113.1 ΔSsys>0, ΔSsurr>0 ΔSsys<0, ΔSsurr>0 ΔSsys>0, ΔSsurr<0 ΔSsys<0, ΔSsurr<0 SubmitMy AnswersGive Up Part C 2H2(g)+O2(g)→2H2O(g)ΔH∘rxn= -483.6 kJ -483.6 ΔSsys>0, ΔSsurr>0 ΔSsys<0, ΔSsurr>0 ΔSsys>0, ΔSsurr<0 ΔSsys<0, ΔSsurr<0
Calculate ΔSsys, ΔSsurr, and ΔStot when 245 g of ice at 0 oC is added to 32 g of steam at 115 oC in a poorly insulated container. During this addition, 4530 J of heat energy is lost to the surroundings. The values of Cp,m for water, ice, and steam are 75.3 J/K mol, 37.7 J/K mol, and 35.5 J/K mol respectively. The ΔHfus for water is 6.02 kJ/mol and the ΔHvap for water is 40.656 kJ/mol.
When one mole of liquid water is frozen in a freezer at –10°C, what are the relative values of ΔSsys and ΔSsurr? Is the reaction spontaneous? ΔSsys < 0, ΔSsurr > 0, spontaneous ΔSsys > 0, ΔSsurr < 0, equilibrium ΔSsys > 0, ΔSsurr < 0, non-spontaneous ΔSsys < 0, ΔSsurr > 0, non-spontaneous ΔSsys > 0, ΔSsurr < 0, spontaneous
Explain the answer A closed system experiences a process such that ΔSsys< 0. From this information, we can conclude: The process was isothermal. The process was non-adiabatic. The process was irreversible. The process was impossible.
For a spontaneous process, which of the following MUST be true? (select all that apply) Select all that apply: TΔS>ΔH ΔG>0 ΔSuniv>0 ΔSsys>ΔSsurr
For the following reaction, N2 (g) + 1/2O2 (g) N2O (g) At 298 K, ΔSsurr = - 275.34 J/K and ΔSsys = -74.3 J/K. Which of the following statements is true? ΔSuniv = -201.04 J/K and the process is nonspontaneous at 298K ΔSuniv = -201.04 J/K and the process is spontaneous at 298K ΔSuniv = 201.04 J/K and the process is spontaneous at 298K ΔSuniv = -349.6 J/K and the process is nonspontaneous at 298K ΔSuniv = -349.6 J/K and the process...
For the following reaction, at 25 °C (room temperature), what is the entropy change of the system? H2O(l) → H2O(s). A) ΔSsys < 0 B) ΔSsys > 0 C) ΔSsys = 0 ----------------------------------------------------------------------------------------------------------------------------- For the following reaction, at 25 °C (room temperature), what is the entropy change of the surroundings? H2O(l) → H2O(s) A) ΔSsurr < 0 B) ΔSsurr = 0 C) ΔSsurr > 0 ---------------------------------------------------------------------------------------------------------- For the following reaction, at 25 °C (room temperature), what is the entropy change...
For a process to be at equilibrium, it is necessary that A. AS(sys) = AS(surr) B. AS(sys) =- AS(surr) OC. AS(total) = 0 OD.B and C are correct
What is ΔSsys for a melting phase transition at 10.2 °C for a compound that melts at 10.2 °C and the ΔHsys = 5.98 kJ mol-1 for this process?
What is ΔSsys for a condensation phase transition at 40.6 °C for a compound that condenses at 40.6 °C and the ΔHsys = -88.1 kJ mol-1 for this process?