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)?

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?

Give the Kirchhoff's equation at constant volume.

Which of the following is not the equation of Kirchhoff's law?

Which law relates the temperature and enthalpy change of a reaction?