Match the following parameters with a description for spontaneity.

\(\Delta\) (Parameters) \(\Delta r\ H^⊝\) \(\Delta r\ S^⊝\)\(\Delta r\ G^⊝\)	Description
A. + - +	1. Non-spontaneous at high temperature
B. - - + at high T	2. Spontaneous at all temperatures
C. - + -	3. Non-spontaneous at all temperatures

Codes

	A	B	C
1.	3	1	2
2.	1	2	3
3.	1	3	2
4.	3	2	1

 Match the following:

Codes

           A            B          C           D

1.       2, 4         2           3            1

2.        1            2           3            4

3.        1           4, 3        3            2

4.       4             3          3, 1         2

Assertion: Combustion of all organic compounds is an exothermic reaction.

Reason: The enthalpies of all elements in their standard state are zero.

1.  Both assertion and reason are true and the reason is the correct explanation of assertion.

2.  Both assertion and reason are true and the reason is not the correct explanation of assertion.

3.  Assertion is true but the reason is false.

4.  Assertion is false but the reason is true.

Assertion: Spontaneous process is an irreversible process and may be reversed by some external agency.

Reason: A decrease in enthalpy is a contributing factor to spontaneity.

1.  Both assertion and reason are true and the reason is the correct explanation of assertion.

2.  Both assertion and reason are true but the reason is not the correct explanation of assertion.

3.  Assertion is true but the reason is false.

4.  Assertion is false but the reason is true.

Assertion: A liquid crystallises into a solid and is accompanied by a decrease in entropy.

Reason: In crystals, molecules organise in an ordered manner.

1.  Both assertion and reason are true and the reason is the correct explanation of assertion.

2.  Both assertion and reason are true but the reason is not the correct explanation of assertion.

3.  Assertion is true but the reason is false.

4.  Assertion is false but the reason is true.

Thermodynamics is not concerned about-

1. Energy changes involved in a chemical reaction

2. The extent to which a chemical reaction proceeds

3. The rate at which a reaction proceeds

4. The feasibility of a chemical reaction

The correct statement among the following is-

1. The presence of reacting species in a covered beaker is an example of an open system.

2. There is an exchange of energy as well as matter between the system and the surroundings in a closed system.

3. The presence of reactants in a closed vessel made up of copper is an example of a closed system.

4. The presence of reactants in a thermos flask or any other closed insulated vessel is an example of a closed system.

If the volume of a gas is reduced to half from its original volume, then the specific heat will-

1.  Reduce to half

2.  Be Doubled

3.  Remain constant

4.  Increase four times

During complete combustion of one mole of butane, 2658 kJ of heat is released. The thermochemical reaction for this change is -

1. $$\begin{gathered} 2{\mathrm{C}}_4{\mathrm{H}}_{10}\left(\mathrm{g}\right)+13{\mathrm{O}}_2\left(\mathrm{g}\right)\to 8{\mathrm{CO}}_2\left(\mathrm{g}\right)+10{\mathrm{H}}_2\mathrm{O}\left(\mathrm{l}\right); \\ {∆}_{\mathrm{c}}\mathrm{H}=-2658.0 \mathrm{kJ} {\mathrm{mol}}^{-1} \end{gathered}$$

2. $$\begin{gathered} {\mathrm{C}}_4{\mathrm{H}}_{10}\left(\mathrm{g}\right)+\frac{13}{2}{\mathrm{O}}_2\left(\mathrm{g}\right)\to 4{\mathrm{CO}}_2\left(\mathrm{g}\right)+5{\mathrm{H}}_2\mathrm{O}\left(\mathrm{l}\right); \\ {∆}_{\mathrm{c}}\mathrm{H}=-1329.0 \mathrm{kJ} {\mathrm{mol}}^{-1} \end{gathered}$$

3. $$\begin{gathered} {\mathrm{C}}_4{\mathrm{H}}_{10}\left(\mathrm{g}\right)+\frac{13}{2}{\mathrm{O}}_2\left(\mathrm{g}\right)\to 4{\mathrm{CO}}_2\left(\mathrm{g}\right)+5{\mathrm{H}}_2\mathrm{O}\left(\mathrm{l}\right); \\ {∆}_{\mathrm{c}}\mathrm{H}=-2658.0 \mathrm{kJ} {\mathrm{mol}}^{-1} \end{gathered}$$

4. $$\begin{gathered} {\mathrm{C}}_4{\mathrm{H}}_{10}\left(\mathrm{g}\right)+\frac{13}{2}{\mathrm{O}}_2\left(\mathrm{g}\right)\to 4{\mathrm{CO}}_2\left(\mathrm{g}\right)+5{\mathrm{H}}_2\mathrm{O}\left(\mathrm{l}\right); \\ {∆}_{\mathrm{c}}\mathrm{H}=+2658.0 \mathrm{kJ} {\mathrm{mol}}^{-1} \end{gathered}$$

${∆}_{\mathrm{f}}{\mathrm{U}}^{⊝}$ of formation of ${\mathrm{CH}}_4\left(\mathrm{g}\right)$ at certain temperature is $-393 \mathrm{kJ} {\mathrm{mol}}^{-1}$. The value of ${∆}_{\mathrm{f}}{\mathrm{H}}^{⊝}$ is-

1. Zero

2. $<{∆}_{\mathrm{f}}{\mathrm{U}}^{⊝}$

3. $>{∆}_{\mathrm{f}}{\mathrm{U}}^{⊝}$

4. Equal to ${∆}_{\mathrm{f}}{\mathrm{U}}^{⊝}$