Thermodynamics ...

For the reaction : $$X_2O_4(l)\rightarrow 2XO_2(g)$$. $$\Delta U = 2.1\,kcal,\  \Delta S = 20\,cal\,K^{ -1 }\,at\ 300\,K$$. 
Hence $$\Delta G$$ is:

$$C(s) + O_2(g)  \rightarrow  CO_2(g),  \quad \Delta{H} = + 94.0  K cal.$$

200 ml of 1M HCl is mixed with 400 ml of 0.5M NaOH. The temperature rise in the calorimeter was found to be 4.0oC. Water equivalent of calorimeter is 25g and the specific heat of the solution is 1 cal/mL/degree. If the theoritical heat of neutralization of a strong acid and strong base is −13.5 kcal, then the percentage error  in this experiment while calculating the heat of neutralization is

0.16 g of methane was subjected to combustion at $$27^{\circ}C$$ in bomb calorimeter. The temperature of calorimeter system (including water)  was found to rise by $$0.5^{\circ}C$$. If the heat of combustion of methane at constant volume and constant pressure is $$x$$ kJ/mole, find the value of $$x$$. The thermal capacity of the calorimeter system is $$17.7\ kJ\ K^{-1},\ R=8.314\ JK^{-1}\ mol^{-1}$$.

For the hypothetical reaction: 
   $${ A }_{ 2 }(g)+{ B }_{ 2 }(g)\rightleftharpoons 2AB(g)$$

$${ \Delta  }_{ r }{ G }^{ o }$$ and $${ \Delta  }_{ r }{ S }^{ o }$$ is $$20 kJ/mol$$ and $$-20{ JK }^{ -1 }{ mol }^{ -1 }$$ respectively at $$200K$$. If $${ \Delta  }_{ r }{ C  }_{ p }$$ is $$20{ JK }^{ -1 }{ mol }^{ -1 }$$ then $${ \Delta  }_{ r }{ H }^{ o }$$ at $$400K$$ is :

Specific heat of substance at m.pt. (or b.pt. or for isothermal process) and specific heat of a substance during adiabatic change respectively are

The heat of reaction for $$A + \frac{1}{2} O_2  \rightarrow AO$$ is $$-50$$ kcal/mol and $$AO + \frac{1}{2} O_2  \rightarrow AO_2$$ is $$100$$ kcal/mol.
The heat of reaction (in kcal/mol) for $$A + O_2  \rightarrow AO_2$$ will be:

Combustion of surose is used by aerobic organisms for providing energy for the life sustaining processes. If all the capturing of energy from the reaction is done through electrical process (non P-V work) then calculate maximum available energy which can be captured by combustion of $$34.2gm$$ of sucrose
Given : $$\Delta {{H}_{combustion}}(sucrose)=-6000\ kJ. {mol}^{-1}$$
             $$\Delta {{S}_{combustion}}=180J/K.mol$$ and body temperature is $$300K$$

Find the forward$$\displaystyle \:\Delta _{r}U^{\circ}$$ at 300K for the reaction  $$4HCl(g)+O_{2}(g)\rightarrow 2Cl_{2}(g)+2H_{2}O(g)$$ Assume all gases are ideal. Given $$\displaystyle \:H_{2}(g)+Cl_{2}(g)\rightarrow 2HCl(g)$$ $$\Delta _{r}H_{300}^{^{\circ}}= -184.5 kJ/mol$$ 
$$\displaystyle \:2H_{2}(g)+O_{2}(g)\rightarrow 2H_2O(g)$$ $$\Delta _{r}H_{300}^{^{\circ}}= -483 kJ/mol$$ (Use R= 8.3 J/mole)

In the Born-Haber cycle for the formation of solid common salt ($$Nacl$$), the largest contribution comes from