Enthalpies for Different Types of Reactions

Enthalpy of neutralisation of acetic acid by $\mathrm{NaOH}$ is $50.6 \mathrm{kJ}/\mathrm{mol}$. Calculate $∆\mathrm{H}$ for ionisation of ${\mathrm{CH}}_3\mathrm{COOH}$. Given the heat of neutralisation of a strong acid with a strong base is $-55.9 \mathrm{kJ}/\mathrm{mol}$.

$5$ litre water at$100$ degree Celsius is mixed with $10$ litre cold water at $10$ degrees Celsius for bath. The final temperature of water is.

The enthalpy changes at $298 \mathrm{K}$ in successive breaking of $\mathrm{O}-\mathrm{H}$ bonds of water are-
${\mathrm{H}}_2\mathrm{O} \to \mathrm{H}\left(\mathrm{g}\right)+\mathrm{OH}\left(\mathrm{g}\right); ∆\mathrm{H}= 498 \mathrm{kJ} {\mathrm{mol}}^{-1}$
$\mathrm{OH} \to \mathrm{H}\left(\mathrm{g}\right)+\mathrm{O}\left(\mathrm{g}\right); ∆ \mathrm{H}= 428 \mathrm{kJ} {\mathrm{mol}}^{-1}$
The bond enthalpy of $\mathrm{O}-\mathrm{H}$ bond is
 

From the reactions:

$\mathrm{C}\left(\mathrm{s}\right)+2{\mathrm{H}}_2\left(\mathrm{g}\right)\to {\mathrm{CH}}_4\left(\mathrm{g}\right),\mathrm{\Delta H}=- \mathrm{X} \mathrm{kCal}$

$\mathrm{C}\left(\mathrm{g}\right)+4\mathrm{H}\left(\mathrm{g}\right)\to {\mathrm{CH}}_4\left(\mathrm{g}\right),\mathrm{\Delta H}=- {\mathrm{X}}_1 \mathrm{kCal}$

${\mathrm{CH}}_4\left(\mathrm{g}\right)\to {\mathrm{CH}}_3\left(\mathrm{g}\right)+\mathrm{H}\left(\mathrm{g}\right),\mathrm{\Delta H}=+ \mathrm{Y} \mathrm{kCal}$

Bond energy of $\mathrm{C}-\mathrm{H}$ bond is:

A natural gas was containing mixture of methane and ethane only. On complete combustion of $10$ litres of gas at STP, the heat evolved was $474.6 \mathrm{kJ}$. Assuming $∆{\mathrm{H}}_{\mathrm{comb}}{\mathrm{CH}}_4\left(\mathrm{g}\right)=-894 \mathrm{kJ}/\mathrm{mol}$ and $∆{\mathrm{H}}_{\mathrm{comb}}{\mathrm{C}}_2{\mathrm{H}}_6\left(\mathrm{g}\right)=-1500 \mathrm{kJ}/\mathrm{mol}$, the percentage of ${\mathrm{CH}}_4$ and ${\mathrm{C}}_2{\mathrm{H}}_6$ will be respectively

The heat of combustion of glucose is $-2840 \mathrm{kJ} {\mathrm{mol}}^{-1}$. Find volume of ${\mathrm{O}}_2$ gas required for complete combustion at STP if $5.68 \mathrm{kJ}$ heat was released on the combustion of glucose.

When $5$ litres of a gas mixture of methane and propane is perfectly combusted at $0^{\circ }\mathrm{C}$ and $1 \mathrm{atm}$, $16 \mathrm{litres}$ of oxygen at the same temperature and pressure is consumed. The amount of heat released from this combustion in $\mathrm{kJ}$ $\left(∆{\mathrm{H}}_{\mathrm{comb}}\left({\mathrm{CH}}_4\right)=890 \mathrm{kJ} {\mathrm{mol}}^{-1}, ∆{\mathrm{H}}_{\mathrm{comb}}\left({\mathrm{C}}_3{\mathrm{H}}_8\right)=2220 \mathrm{kJ} {\mathrm{mol}}^{-1}\right)$ is :

Correct expression of enthalpy of combustion is :

$24.63 \mathrm{L}$ of ${\mathrm{C}}_2{\mathrm{H}}_4$ gas is burnt at $1 \mathrm{atm}$ pressure and $300 \mathrm{K}$ temperature. If the heat released at constant pressure due to combustion is $280 \mathrm{kJ}$, then calculate heat of combustion of $1 \mathrm{gm}$ of ${\mathrm{C}}_2{\mathrm{H}}_4$ gas.

Standard heat of formation of $\mathrm{KI}$ is $-78.31 \mathrm{kcal}/\mathrm{mol}$. Calculate its lattice energy from following informations : ${\mathrm{I}}_1\left(\mathrm{K}\right)=4.3 \mathrm{eV}$, ${\mathrm{E}}_1\left(\mathrm{I}\right)=-73.4 \mathrm{k} \mathrm{cal}/\mathrm{mol}$

Bond dissociation energy of ${\mathrm{I}}_2$ is $36.1 \mathrm{K} \mathrm{cal}/\mathrm{mol}$, sublimation energy of $\mathrm{K}$ is $21.51 \mathrm{k} \mathrm{cal}/\mathrm{mol}$.

Energy required to dissociate $16 \mathrm{g}$ of oxygen gas into free atoms is $\mathrm{x} \mathrm{kJ}$. The heat of atomization of oxygen is 

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:

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