mark each of True or False. (a) Half-life of a compound decomposing in second order process only

mark each of True or False.

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(a) Half-life of a compound decomposing in second order process only depends on the reaction rate (b) Half-life of a compound decomposing in 0-th order process only depends on the reaction rate (c) If a reaction enthalphy <0 and reaction entropy > 0, the reaction is only spontaneous if temperature is larger than certain temperature T (d) If reaction enthalpy is> 0 and reaction entropy > 0, the reaction is always spontaneous (e) If reaction enthalpy is> 0 and reaction entropy > 0, the reaction is never spontaneous (f) We have a system that can exist in two isomers, A and B, with reaction rate A >>> B equal to ki, and reaction rate of B-> A equal to k₂. To be able to determine he ratio of equilibrium concentrations [A]/[B], we also need to specify the initial concentrations of A and B. (g) Perpetum mobile of the second kind satisfies first law of thermodynamics, but breaks the second law. (h) One of the equivalent formulations of the third law of thermodynamics states it is impossible to reach T=OK. (i) We are studying two different reactions A<B. and C <>D. The Gibbs free energy difference between the starting state and end state of the process are the same, but in one case (C >>> D) the reaction includes much larger barrier during the conversion of C to D. Hence, the equilibrium ratio D/C is going to be smaller than B/A. (j) I have a reaction of compounds in solution, following this reaction: A + B <>C, which reaches its equilibrium concentrations A eq, B_eq, and C eq. Then, I will add some more C to the equilibrated mixture, and let it equilibrate into a new values of concentrations A*_eq, B*_eq, and C*_eq. This is enough information for us to be able to say that A*_eq will be larger than A_eq. (a) Half-life of a compound decomposing in second order process only depends on the reaction rate (b) Half-life of a compound decomposing in 0-th order process only depends on the reaction rate (c) If a reaction enthalphy <0 and reaction entropy > 0, the reaction is only spontaneous if temperature is larger than certain temperature T (d) If reaction enthalpy is> 0 and reaction entropy > 0, the reaction is always spontaneous (e) If reaction enthalpy is> 0 and reaction entropy > 0, the reaction is never spontaneous (f) We have a system that can exist in two isomers, A and B, with reaction rate A >>> B equal to ki, and reaction rate of B-> A equal to k₂. To be able to determine he ratio of equilibrium concentrations [A]/[B], we also need to specify the initial concentrations of A and B. (g) Perpetum mobile of the second kind satisfies first law of thermodynamics, but breaks the second law. (h) One of the equivalent formulations of the third law of thermodynamics states it is impossible to reach T=OK. (i) We are studying two different reactions A<B. and C <>D. The Gibbs free energy difference between the starting state and end state of the process are the same, but in one case (C >>> D) the reaction includes much larger barrier during the conversion of C to D. Hence, the equilibrium ratio D/C is going to be smaller than B/A. (j) I have a reaction of compounds in solution, following this reaction: A + B <>C, which reaches its equilibrium concentrations A eq, B_eq, and C eq. Then, I will add some more C to the equilibrated mixture, and let it equilibrate into a new values of concentrations A*_eq, B*_eq, and C*_eq. This is enough information for us to be able to say that A*_eq will be larger than A_eq.

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