Enthalpies for Different Types of Reactions

From the data of following bond energies:

 $\begin{array}{l}H-Hbondenergy:431.37kJmo{l}^{-1}\\ C=Cbondenergy:606.10kJmo{l}^{-1}\\ C-Cbondenergy:336.49kJmo{l}^{-1}\\ C-Hbondenergy:410.50kJmo{l}^{-1}\end{array}$

Calculate the enthalpy of the following reaction in $kJmo{l}^{-1}$.

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)?

Which one of the following is the correct relation between ${\mathrm{C}}_{\mathrm{P}}$ and ${\mathrm{C}}_{\mathrm{V}}$ for one mole of an ideal gas? ($\mathrm{R}$ is molar gas constant)

The standard enthalpy of formation of ${\mathrm{CH}}_4\left(\mathrm{g}\right),{\mathrm{CO}}_2\left(\mathrm{g}\right)$ and ${\mathrm{H}}_2\mathrm{O}\left(\mathrm{l}\right)$ are $-75 \mathrm{kJ} {\mathrm{mol}}^{-1}$, $-393 \mathrm{kJ} {\mathrm{mol}}^{-1}$ and $-286 \mathrm{kJ} {\mathrm{mol}}^{-1}$ respectively. The amount of heat liberated (in ${\mathrm{kJ}}^2$) when $3.2 \mathrm{g}$ of methane gas is burnt under standard conditions is

$2 \mathrm{moles}$ of a mixture of acetylene and ethane produced on combustion, $5500 \mathrm{kJ}$ of heat energy. The enthalpies of combustion of acetylene and ethane are $2000$ and $3000 \mathrm{kJ} {\mathrm{mol}}^{-1}$ respectively. The ratio of acetylene to ethane in the mixture is

How many of the following have standard heat of formation value of zero.

$\left(\mathrm{i}\right) {\mathrm{Br}}_{2\left(\mathrm{l}\right)}$

$\left(\mathrm{ii}\right) {{\mathrm{CO}}_2}_{\left(\mathrm{g}\right)}$

$\left(\mathrm{iii}\right) {\mathrm{C}}_{\text{(graphite) }}$

$\left(\mathrm{iv}\right) {\mathrm{Cl}}_{2\left(\mathrm{l}\right)}$

$\left(\mathrm{v}\right) {\mathrm{Cl}}_{2\left(\mathrm{g}\right)}$

$\left(\mathrm{vi}\right) {\mathrm{F}}_{2\left(\mathrm{g}\right)}$

$\left(\mathrm{vii}\right) {\mathrm{F}}_{\left(\mathrm{g}\right)}$

$\left(\mathrm{viii}\right) {\mathrm{I}}_{2\left(\mathrm{g}\right)}$

$\left(\mathrm{ix}\right) {\mathrm{S}}_{\left(\text{monoclinic }\right)}$

$\left(\mathrm{x}\right) {\mathrm{N}}_{2\left(\mathrm{g}\right)}$

$\left(\mathrm{xi}\right) {\mathrm{P}}_{\left(\mathrm{blcak}\right)}$

$\left(\mathrm{xii}\right) {\mathrm{P}}_{\left(\mathrm{red}\right)}$

$\left(\mathrm{xiii}\right) {\mathrm{CH}}_4$

In Kirchhoff's equation, the term ${\mathrm{C}}_{\mathrm{v}}$ is used instead of ${\mathrm{C}}_{\mathrm{p}}$ at constant volume.

Kirchhoff's equation at constant volume is : 

The variation of $∆\mathrm{U}$ with temperature is expressed by Kirchoff's equation.

Temperature affects the  enthalpy change of a reaction.

Write the Kirchhoff's equation at constant volume and at constant pressure.

Specific heat capacity is not the parameter that is used to relate the enthalpy of a reaction and temperature.

Describe the effect of temperature on enthalpy of reaction.

What happens to the enthalpy of the system if its temperature increases?