Enthalpy Change of a Reaction

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 number of endothermic process/es from the following is _______.

A. ${\mathrm{I}}_2( \mathrm{g})\to 2\mathrm{I}\left(\mathrm{g}\right)$

B. $\mathrm{HCl}\left(\mathrm{g}\right)\to \mathrm{H}\left(\mathrm{g}\right)+\mathrm{Cl}\left(\mathrm{g}\right)$

C. ${\mathrm{H}}_2\mathrm{O}\left(\mathrm{l}\right)\to {\mathrm{H}}_2\mathrm{O}\left(\mathrm{g}\right)$

D. $\mathrm{C}\left(\mathrm{s}\right)+{\mathrm{O}}_2( \mathrm{g})\to {\mathrm{CO}}_2( \mathrm{g})$

E. Dissolution of ammonium chloride in water

For complete combustion of ethene,
${\mathrm{C}}_2{\mathrm{H}}_4( \mathrm{g})+3{\mathrm{O}}_2( \mathrm{g})\to 2{\mathrm{CO}}_2( \mathrm{g})+2{\mathrm{H}}_2\mathrm{O}\left(\mathrm{l}\right)$
the amount of heat produced as measured in bomb calorimeter is $1406 \mathrm{kJ} {\mathrm{mol}}^{-1}$ at $300 \mathrm{K}$. The minimum value of $\mathrm{T\Delta S}$ needed to reach equilibrium is $(-)$ $\mathrm{kJ}$. (Nearest integer)
Given: $\mathrm{R}=8.3 \mathrm{J} {\mathrm{K}}^{-1} {\mathrm{mol}}^{-1}$

Given below are two statements related to Ellingham diagram :

Statement I : Ellingham diagrams can be constructed for formation of oxides, sulphides and halides of metals.

Statement II : It consists of plots of $\mathrm{\Delta H}°$ vs $\mathrm{T}$ for formation of oxides of elements.

In the light of the above statements, choose the most appropriate answer from the options given below :

The enthalpy change for the adsorption process and micelle formation respectively are

$\mathrm{C}\left(\mathrm{s}\right)+{\mathrm{O}}_2\left(\mathrm{g}\right)\to {\mathrm{CO}}_2\left(\mathrm{g}\right),\mathrm{\Delta H}=+94.0\mathrm{Kcal}.$

$\mathrm{CO}\left(\mathrm{g}\right)+\frac{1}{2}{\mathrm{O}}_2\left(\mathrm{g}\right)\to {\mathrm{CO}}_2\left(\mathrm{g}\right),\mathrm{\Delta H}=-67.7\mathrm{Kcal}.$

From the above reactions find how much heat ($\mathrm{Kcal} {\mathrm{mole}}^{-1}$) would be produced in the following reaction:

$\mathrm{CO}\left(\mathrm{g}\right)+\frac{1}{2}{\mathrm{O}}_2\left(\mathrm{g}\right)\to \mathrm{CO} \left(\mathrm{g}\right)$

$∆\mathrm{H}$ for the reaction,

${\mathrm{A}}_{\left(\mathrm{g}\right)}+{\mathrm{B}}_{\left(\mathrm{g}\right)}\stackrel{}{\to }{\mathrm{AB}}_{\left(\mathrm{g}\right)}$ at $298 \mathrm{K}$ and $1 \mathrm{atm}$ is $-10 \mathrm{kcal}$.

The $∆\mathrm{U}$ for the above conversion would be

The heat change at constant volume for the decomposition of silver oxide is found to be $80.25 \mathrm{kJ}$ . The heat change at constant pressure will be______. 

The value for $△\mathrm{U}$ for the reversible isothermal evaporation of $90 \mathrm{g}$ water at $100 °\mathrm{C}$ will be : $(△{\mathrm{H}}_{\mathrm{vap}} \mathrm{of} \mathrm{water}=40.8\mathrm{kJ} {\mathrm{mol}}^{-1}, \mathrm{R}=8.314 {\mathrm{JK}}^{-1}{\mathrm{mol}}^{-1})$

The heat of combustion of ethylene at $18°\mathrm{C}$ and at constant volume is $-335.8 \mathrm{kcal}$ when water is obtained in liquid state. What is the heat of combustion at constant pressure and at $18°\mathrm{C}$ ?

Calculate $\mathrm{\Delta H}$ (in joules) for ${\mathrm{C}}_{\left(\mathrm{graphite}\right)}\to {\mathrm{C}}_{\left(\mathrm{diamond}\right)}$ from the following data,

${\mathrm{C}}_{(\mathrm{graphite}) }+{\mathrm{O}}_{2\left(\mathrm{g}\right)}\to {\mathrm{CO}}_{2\left(\mathrm{g}\right)}; \mathrm{\Delta H}=-393.5 \mathrm{kJ}$

${\mathrm{C}}_{(\mathrm{diamond}) }+{\mathrm{O}}_{2( \mathrm{g})}\to {\mathrm{CO}}_{2\left(\mathrm{g}\right)}; \mathrm{\Delta H}=-395.4 \mathrm{kJ}$

Nitroglycerine $\left(\mathrm{MW}=227.1\right)$ detonates according to the following equations,

$2{\mathrm{C}}_3{\mathrm{H}}_5{\left({\mathrm{NO}}_3\right)}_3\left(l\right)⟶3 {\mathrm{N}}_2\left(\mathrm{g}\right)+\frac{1}{2}{\mathrm{O}}_2\left(\mathrm{g}\right)+6{\mathrm{CO}}_2\left(\mathrm{g}\right)+5{\mathrm{H}}_2\mathrm{O}\left(\mathrm{g}\right)$

The standard molar enthalpies of formation, ${\mathrm{\Delta H}}_{\mathrm{f}}°$ for all the compounds are given below.

${\mathrm{\Delta H}}_{\mathrm{f}}°\left[{\mathrm{C}}_3{\mathrm{H}}_5{\left({\mathrm{NO}}_3\right)}_3\right]=-364 \mathrm{kJ}/\mathrm{mol}$
${\mathrm{\Delta H}}_{\mathrm{f}}°\left[{\mathrm{CO}}_2\left(\mathrm{g}\right)\right]=-393.5 \mathrm{kJ}/\mathrm{mol}$
${\mathrm{\Delta H}}_{\mathrm{f}}°\left[{\mathrm{H}}_2\mathrm{O}\left(\mathrm{g}\right)\right]=-241.8 \mathrm{kJ}/\mathrm{mol}$
${\mathrm{\Delta H}}_{\mathrm{f}}°\left[{\mathrm{N}}_2\left(\mathrm{g}\right)\right]=0 \mathrm{kJ}/\mathrm{mol}$
${\mathrm{\Delta H}}_{\mathrm{f}}°\left[{\mathrm{O}}_2\left(\mathrm{g}\right)\right]=0 \mathrm{kJ}/\mathrm{mol}$

The enthalpy change when $10 \mathrm{g}$ of nitroglycerine is detonated is

Which of the following is endothermic reaction :-

The difference between heat of reaction at constant pressure $\left(∆\mathrm{H}\right)$ and at constant volume $\left(\mathrm{\Delta E}\right)$ for the reaction: ${\mathrm{C}}_{\left(\mathrm{s}\right)}+\frac{1}{2}{\mathrm{O}}_{2\left(\mathrm{g}\right)}⟶{\mathrm{CO}}_{\left(\mathrm{g}\right)}$ at a temperature $=\mathrm{T} \mathrm{K}$ is 

(Assume $\mathrm{R}=0.002 \mathrm{kcal} {\mathrm{K}}^{-1}{\mathrm{mol}}^{-1}$)

Define enthalpy of chemical reactions. What is meant by standard state of a substance and standard enthalpy of reactions?