Thermodynamics ...

The value of $$\Delta H$$ and $$\Delta S$$ for a reaction are respectively $$30kJ$$ $${mol}^{-1}$$ and $$100J{K}^{-1}$$ $${mol}^{-1}$$. Then temperature above which the reaction will become spontaneous is:

Which of the following thermodynamics relation is correct?

$$\Delta H$$ and$$\Delta S$$ for the reaction
$${ Br }_{ 2 }(l)+{ Cl }_{ 2 }(l)\longrightarrow 2BrCl(g)$$
are $$29.37\ kJ$$ and $$104.0\ J{ K }^{ -1 }$$ respectively. Above that temperature will this reaction become spontaneous?

A $$1g$$ sample of substance $$A$$ at $${100}^{o}C$$ is added to $$100mL$$ of $${H}_{2}O$$ at $${25}^{o}C$$. Using separate $$100mL$$ portion of $${H}_{2}O$$ the procedure is repeated with substance $$B$$ then with substance $$C$$. How will the final temperatures of the water compare?

The Haber's process for production of ammonia involves the equilibrium:
$${N}_{2}(g)+3{H}_{2}(g)\rightleftharpoons  2{NH}_{3}(g)$$
Assuming $$\Delta {H}^{o}$$ and $$\Delta {S}^{o}$$ for the reaction do not change with temperature, which of the statements is true?
($$\Delta {H}^{o}=-95kJ$$ and $$\Delta {S}^{o}=-190J{ K }^{ -1 }$$)

For a particular reaction, $$\Delta { H }^{ o }=-38.3\ kJ$$ and $$\Delta { S }^{ o }=-113\ J{ K }^{ -1 }{ mol }^{ -1 }$$. This reaction is:

Following enthalpy changes are given:

For which process will $$\Delta { H }^{ o }$$ and $$\Delta { G }^{ o }$$ be expected to be most similar?

Consider the values of $$\Delta { H }^{ o }$$ (in $$kJ{ mol }^{ -1 }$$) and for $$\Delta { S }^{ o }$$ (in $$J{ mol }^{ -1 }{ K }^{ -1 }$$) given for four different reactions. For which reaction will $$\Delta { G }^{ o }$$ increase the most positive) when temperature is increased from $${0}^{o}C$$ to $${25}^{o}C$$?

The standard Gibbs free energy $$\Delta { G }^{ o }$$ is related to equilibrium constant $${K}_{P}$$ as: