Thermodynamics ...

A solution of $$500\ ml$$ of $$2\ M-KOH$$ is added to $$500\ ml$$ of $$2\ M-HCl$$ and the mixture is well shaken. The rise in temperature $$T_{1}$$ is noted. The experiment is again performed using $$250\ ml$$ of  each solution and rise in temperature $$T_{2}$$ is again noted. Which of the following is correct?

The standard heat of combustion of propane is $$-2220.1\ kJ/mol$$. The standard heat of vaporization of liquid water is $$44\ kJ/mol$$. What is the $$\triangle H^{o}$$ of the reaction :
$$C_{3} H_{8} (g)+ 5O_{2} (g) \rightarrow 3CO_{2} (g) + 4H_{2} O (g)$$?

For a specific work, on an average a person requires $$5616\ kJ$$ of energy. How many kilogram of glucose must be consumed if all the require energy has to be derive from glucose only? $$\Delta H$$ for combustion of glucose is $$-2808\ kJ\ mol^{-1}$$

The value of $$\triangle H_{sol}$$ of anhydrous copper $$(II)$$ sulfate is $$-66.11\ kJ.$$ Dissolution of $$1$$ mole of blue vitriol (Copper $$(II)$$ sulphate pentahydrate) is followed by absorption of $$11.5\ kJ$$ of heat. The enthalpy of dehydration of blue vitriol is: 

The data below refers to gas phase reaction at constant pressure at $$25^{o}C.$$
$$CH_{3}- CH_{3} \Rightarrow CH_{3}- CH_{2}+ H; \triangle H_{1} = +420\ kJ\ mol^{-1}$$
$$CH_{3}- CH_{2} \rightarrow CH_{2} = CH_{2}+ H; \triangle H_{2}+ 168\ kJ\ mol^{-1}$$
From these data, the enthalpy change $$\triangle H$$ for the reaction : $$2CH_{3} - CH_{2} \rightarrow CH_{3}- CH_{3}+ CH_{2} = CH_{2}$$ is 

Geological condition are sometimes so extreme that quantities neglected in normal laboratory experiments take on an overriding importance. For example, consider the formation of diamond under geophysically typical conditions. The density of graphite is $$2.4\ g/cm^{3}$$ and that of diamond is $$3.6\ g/cm^{3}$$ at a certain temperature and $$500\ kbar$$. By how much does $$\Delta U_{trans}$$ differes from $$\Delta H_{trans}$$ for the graphite to diamond transition?

The standard enthalpies of formation of $$H_{2}O (l), Li^{+}(aq)$$ and $$OH^{-} (aq)$$ are $$-285.8, -278.5$$ and $$-228.9\ kJ/mol$$, respectively. The standard enthalpy change for the reaction is:

A quantity that cannot be directly measured is:

Enthalpy of  neutralization of oxalic acid is $$-25.4\ kcal/mol$$ using strong base, $$NaOH$$. Enthalpy change for the process:
$$H_{2}C_{2}O_{4}(aq)\rightarrow 2H^{+}(aq)+C_{2}O_{4}^{2-}(aq)$$ is about

For a spontaneous process: