Thermodynamics ...

For a non-spontaneous reaction, at $${30}^{o}C$$, $$\Delta H> 0$$ and $$\Delta S> 0$$. The reaction becomes spontaneous by?

Ethyl chloride ($${C}_{2}{H}_{5}Cl$$) is prepared by reaction of ethylene with hydrogen cloride:
$${C}_{2}{H}_{4}(g)+Hcl(g)\rightarrow {C}_{2}{H}_{5}Cl(g)$$; $$\Delta H=-72.3kJ$$
What is the value of $$\Delta E$$ (in kJ), if $$70g$$ of ethylene and $$73g$$ of $$HCl$$ are allowed to react at $$300K$$

$$\Delta S$$ for $$4Fe(s)+3{O}_{2}(s)\rightarrow 2{Fe}_{2}{O}_{3}(s)$$ is $$-550J/mol/K$$. The process is found to be spontaneous even at $$298K$$ because  ($$\Delta H=-1650kJ$$)

In which of the following case entropy decreases-

For a reaction $${R}_{1},\Delta G=x KJ {mol}^{-1}$$. For a reaction $${R}_{2},\Delta G=y$$ $$KJ{mol}^{-1}$$. Reaction $${R}_{1}$$ is non spontaneous but along with $${R}_{2}$$ it is spontaneous. This means that:

An equilibrium reaction $$X+Y \rightleftharpoons W+Z, \triangle H=+ve $$ is spontaneous in the forward direction. Then corresponding sign of $$\triangle G$$ and $$\triangle S $$ should be respectively:

Rank the following substances in order of decreasing heat of combusion (maximum $$\to$$ minimum). 

Consider the reaction:

In an insulated container 1 mole of a liquid. molar volume 100 ml at 1 bar. Liquid is steeply taken to 100 bar, when volume of liquid decreases by 1 ml. Find $$\Delta H$$ for the process.

the above reaction was carried out at 300 K in a bomb calorimeter. The heat released was 743 kJ/mol. The value of $$\triangle H_{300K}$$ for this reaction would be: