Enthalpies for Different Types of Reactions

What is the enthalpy change for,

$2{\mathrm{H}}_2{\mathrm{O}}_2\left(\mathrm{l}\right)\to 2{\mathrm{H}}_2\mathrm{O}\left(\mathrm{l}\right)+{\mathrm{O}}_2\left(\mathrm{g}\right)$ if heat of formation of  ${\mathrm{H}}_2{\mathrm{O}}_2\left(\mathrm{l}\right)\mathrm{and}{\mathrm{H}}_2\mathrm{O}\left(\mathrm{l}\right)$  are $-188$ and $-286 \mathrm{kJ}/\mathrm{mol}$respectively (in standard conditions)?

The enthalpy change that accompanies melting of one mole of a solid substance in standard state is called enthalpy of atomization.

What is the difference between heat of solution and heat of dilution?

The integral heat of dilution is viewed on a macro scale.

The _____ heat/enthalpy of dilution is viewed on a micro scale.

A gas mixture of $3.67 \mathrm{L}$ of ethylene and methane on complete combustion at $25°\mathrm{C}$ and at $1 \mathrm{atm}$ pressure produce $6.11 \mathrm{L}$ of carbon dioxide. Find out the amount of heat evolved in $\mathrm{kJ}$, during this combustion. $(∆{\mathrm{H}}_{\mathrm{c}}({\mathrm{CH}}_4)=-890 {\mathrm{kJmol}}^{-1}$ and $∆{\mathrm{H}}_{\mathrm{c}}\left({\mathrm{C}}_2{\mathrm{H}}_4\right)=-1423 {\mathrm{kJmol}}^{-1})$

The lattice enthalpy and hydration enthalpy of four compounds are given below:

The pair of compounds which is soluble in water is

The amount of energy released in burning $1\mathrm{kg}$ of coal is

Match the column I with column II and mark the appropriate choice.

Calculate$\mathrm{C}-\mathrm{Cl}$bond enthalpy from the following data:

${\mathrm{CH}}_3\mathrm{CI} \left(\mathrm{g}\right) + {\mathrm{CI}}_2 \left(\mathrm{g}\right) \to {\mathrm{CH}}_2{\mathrm{CI}}_2 \left(\mathrm{g}\right) + \mathrm{HCl} \left(\mathrm{g}\right) ∆\mathrm{H}° = -104 \mathrm{kJ}$

$$\begin{gathered} \mathrm{Bond} \mathrm{C}-\mathrm{H} \mathrm{Cl}-\mathrm{Cl} \mathrm{H}-\mathrm{Cl} \\ ∆\mathrm{H}/\mathrm{kJ} {\mathrm{mol}}^{-1} 414 243 431 \end{gathered}$$

Calculate$∆\mathrm{H}°$ of the reaction

${\mathrm{CH}}_4\left(\mathrm{g}\right)+{\mathrm{O}}_2\left(\mathrm{g}\right)\to {\mathrm{CH}}_2\mathrm{O}\left(\mathrm{g}\right)+{\mathrm{H}}_2\mathrm{O}\left(\mathrm{g}\right)$ from the following data:

$$\begin{gathered} \mathrm{Bond} \mathrm{C}-\mathrm{H} O = O \mathrm{C} = \mathrm{O} \mathrm{O}-\mathrm{H} \\ ∆\mathrm{H}°{\mathrm{kJmol}}^{-1} 414 499 745 464 \end{gathered}$$

What is meant by bond enthalpy? How is it useful to calculate reaction enthalpy? Explain with one example.
 

Explain standard enthalpy of combustion with an example.
 

Define and explain enthalpy of atomization with an example.

Calculate the enthalpy change for the reaction,

${\mathrm{H}}_2\mathrm{O}\left(\mathrm{g}\right)⟶2\mathrm{H}\left(\mathrm{g}\right)+\mathrm{O}\left(\mathrm{g}\right)$ and hence, calculate the bond enthalpy of $O-\mathrm{H}$
bond in ${\mathrm{H}}_2\mathrm{O}$ from the following data;

${\mathrm{\Delta }}_{\mathrm{vap}}\mathrm{H}\left({\mathrm{H}}_2\mathrm{O}\right)=44.0{\mathrm{kJmol}}^{-1}$

${\mathrm{\Delta }}_{\mathrm{f}}\mathrm{H}\left({\mathrm{H}}_2\mathrm{O}\right)=-285.8{\mathrm{kJmol}}^{-1}$

$\begin{array}{l}{\Delta }_{\mathrm{a}}\mathrm{H}\left({\mathrm{H}}_2\right)=436.0{\mathrm{kJmol}}^{-1},{\Delta }_{\mathrm{a}}\mathrm{H}\left({\mathrm{O}}_2\right)=498.0\mathrm{kJ}\\ {\mathrm{mol}}^{-1}\end{array}$

where ${∆}_{\mathrm{a}}\mathrm{H}$ is the enthalpy of atomization.
 

Calculate, using the data given in the table below, the enthalpy of the reaction,
${\mathrm{CH}}_3\mathrm{COOH} \left(\mathrm{g}\right) + {\mathrm{CH}}_3{\mathrm{CH}}_2\mathrm{OH}\left(\mathrm{g}\right) \to {\mathrm{CH}}_3{\mathrm{COOCH}}_2{\mathrm{CH}}_3\left(\mathrm{g}\right)+{\mathrm{H}}_2\mathrm{O}\left(\mathrm{g}\right)$

The standard enthalpy of combustion at $25°\mathrm{C}$ of hydrogen, cyclohexane $\left({\mathrm{C}}_6{\mathrm{H}}_{10}\right)$ and cyclohexane $\left({\mathrm{C}}_6{\mathrm{H}}_{12}\right)$ are $–241, –3800$ and $–3920 \mathrm{kJ}/\mathrm{mol}$ respectively. Calculate the heat of hydrogenation of cyclohexane.

Select the incorrect statement(s) from the following:

Given, ${\text{N}}_2\left(\text{g}\right)+3{\text{H}}_2\left(\text{g}\right)\to 2{\text{NH}}_3\left(\text{g}\right)\text{;}{\Delta }_{\text{r}}{\text{H}}^{\circ }=-92·4\text{kJ}{\text{mol}}^{-1}$

What is the standard enthalpy of formation of NH₃ gas in KJ mole^-1.

One mole of methanol, when burnt in oxygen, gives out 723 kJ $\mathrm{m}\mathrm{o}{\mathrm{l}}^{-1}$ heat. If one mole of oxygen is used, what will be the amount of heat evolved?