$$\Delta S$$ [ change in entropy ] and $$\Delta H$$ [ change in enthalpy ] are related by the equation $$\Delta G = \Delta H - T\Delta S$$
[ Here, $$\Delta G = $$ change in Gibbs free energy ]
For adsorption of a gas, $$\Delta S$$ is negative because randomness decreases. Thus, in order to make $$\Delta G$$ negative [ for spontaneous reaction ], $$\Delta H$$ must be highly negative. Hence for the adsorption of a gas, if $$\Delta S$$ is negative, therefore, $$\Delta H$$ should be highly negative.
3.
If the bond energies of $$H-H,$$ $$Br-Br$$ and $$H-Br$$ are $$433, 192$$ and $$364\,kJ\,mo{l^{ - 1}}$$ respectively, then $$\Delta {H^ \circ }$$ for the reaction $${H_2}\left( g \right) + B{r_2}\left( g \right) \to 2HBr\left( g \right)$$ is
4.
Following reaction occurrs in an automobile $$2{C_8}{H_{18}}\left( g \right) + 25{O_2}\left( g \right) \to 16C{O_2}\left( g \right) + 18{H_2}O\left( g \right).$$ The sign of $$\Delta H,\Delta S$$ and $$\Delta G$$ would be
For combustion reaction, $$\Delta H$$ is negative, $$\Delta n = \left( {16 + 18} \right) - \left( {25 + 2} \right) = + 7,$$ so $$\Delta S$$ is $$ + ve,$$ reaction is spontaneous, hence $$\Delta G$$ is $$ - ve.$$
5.
In a reaction $$P + Q \to R + S,$$ there is no change in entropy. Enthalpy change for the reaction $$\left( {\Delta H} \right)$$ is $$12\,kJ\,mo{l^{ - 1}}.$$ Under what conditions, reaction will have negative value of free energy change ?
Work is not a state function because it depends upon the path followed.
7.
A gas undergoes change from state $$A$$ to state $$B.$$ In this process, the heat absorbed and work done by the gas is $$5\,J$$ and $$8\,J,$$ respectively. Now gas is brought back to $$A$$ by another process during which $$3\,J$$ of heat is evolved. In this reverse process of $$B$$ to $$A$$ :
A.
$$10\,J$$ of the work will be done by the gas.
B.
$$6\,J$$ of the work will be done by the gas.
C.
$$10\,J$$ of the work will be done by the surrounding on gas.
D.
$$6\,J$$ of the work will be done by the surrounding on gas.
Answer :
$$6\,J$$ of the work will be done by the surrounding on gas.
$$\eqalign{
& \Delta {U_{AB}} = q + w = + 5 + \left( { - 8} \right) = - 3 \cr
& q = - 3,\,\Delta {U_{BA}} = + 3 \cr
& \,\Delta {U_{BA}} = q + w \cr
& \Rightarrow 3 = - 3 + w \Rightarrow w = + 6\,J\,{\text{(work done on the system)}}{\text{.}} \cr} $$
8.
If the bond dissociation energies of $$XY,{X_2}$$ and $${Y_2}$$ ( all
diatomic molecules ) are in the ratio of 1 : 1 : 0.5 and $$\Delta {H_f}$$ for the formation of $$XY$$ is $$ - 200\,kJ\,mo{l^{ - 1}}.$$ The bond dissociation energy of $${X_2}$$ will be
10.
Two reactions are given below :
$$\eqalign{
& \left( {\text{i}} \right)C{O_{\left( g \right)}} + \frac{1}{2}{O_{2\left( g \right)}} \to C{O_{2\left( g \right)}} \cr
& \left( {{\text{ii}}} \right)A{g_2}{O_{\left( s \right)}} \to 2A{g_{\left( s \right)}} + \frac{1}{2}{O_{2\left( g \right)}} \cr} $$
Which of the following statements is true ?
A.
For $$\left( {\text{i}} \right)\Delta H < \Delta U$$ and for $$\left( {{\text{ii}}} \right)\Delta H > \Delta U$$
B.
For $$\left( {\text{i}} \right)\Delta H > \Delta U$$ and for $$\left( {{\text{ii}}} \right)\Delta H < \Delta U$$
C.
For both $$\left( {\text{i}} \right)$$ and $$\left( {{\text{ii}}} \right)\Delta H > \Delta U$$
D.
For both $$\left( {\text{i}} \right)$$ and $$\left( {{\text{ii}}} \right)\Delta H < \Delta U$$
Answer :
For $$\left( {\text{i}} \right)\Delta H < \Delta U$$ and for $$\left( {{\text{ii}}} \right)\Delta H > \Delta U$$