An enthalpy diagram for a particular reaction is given below:

Which of the following statements is correct?

1.	Reaction is spontaneous
2.	Reaction is non-spontaneous
3.	The spontaneity of the reaction cannot be determined from the graph provided above.
4.	None of the above

What is the nature of the reaction depicted in the given diagram for A→C?

Consider the following diagram for a reaction $\mathrm{A}\to \mathrm{C}$. 

The nature of the reaction is-

1. Exothermic

2. Endothermic

3. Reaction at equilibrium

4. None of the above

Consider the following graph.

The work done, as per the graph above, is:

For the graph given below, it can be concluded that work done during the process shown will be:

What is the entropy change of the surroundings when 1.00 mol of liquid water (H₂O(l)) is formed under standard conditions?
[Given: ∆_fH^θ = –286 kJ mol^–1 ]

1. 952. 5 J mol^-1

2. $979.7$ $\mathrm{J}$ ${\mathrm{mol}}^{-1}$

3. $949.7$ $\mathrm{J}$ ${\mathrm{mol}}^{-1}$

4. $959.7$ $\mathrm{J}$ ${\mathrm{mol}}^{-1}$

Find the thermodynamic stability of NO(g) relative to NO₂(g) using the following data:

½N₂(g) + ½O₂(g) → NO(g)  ΔrH° = +90 kJ mol⁻¹

NO(g) + ½O₂(g) → NO₂(g)  ΔrH° = −74 kJ mol⁻¹
1. Less than NO₂(g)
2. More than NO₂(g)
3. Equal to NO₂(g)
4. Insufficient data

The difference between enthalpy (∆H) and internal energy (∆E) for the given below reaction,
under constant temperature, is:
\(C_{3} H_{8} \left(\right. g \left.\right) + 5 O_{2} \left(\right. g \left.\right) \rightarrow 3 CO_{2} \left(\right. g \left.\right) + 4 H_{2} O \left(\right. l \left.\right)\)

For the given reaction 

$2H_2{O}_2\left(l\right)$ $\to$ $2H_{2}O\left(l\right)$ $+$ $O_2\left(g\right)$, the heat of formations of ${\mathrm{H}}_2{\mathrm{O}}_2\left(\mathrm{l}\right)$ $$ $\mathrm{and}$ ${\mathrm{H}}_2\mathrm{O}$ $\left(\mathrm{l}\right)$ $$are -188 kJ/mol & -286 KJ/mol respectively. The change in the enthalpy of the reaction will be:

1.  – 196 kJ/mol

2.  + 196 kJ/mol

3.  + 948 kJ/mol

4.  – 948 kJ/mol