What is true for a cyclic process:

1.  a, b
2.  b, c
3.  c, d
4.  a, d

If a system is expanded under adiabatic process, then:

1.  Temperature increases
2.  ∆E decreases
3.  ∆E increases
4.  None of the above

Which of the following is true for a reaction in which all the reactants & products are liquids:
1.  ∆H = ∆E
2.  ∆H = ∆W
3.  ∆H > ∆E
4.  None of the above

For the reaction
C₂H₅OH(l) + 3O₂(g) →2CO₂(g) + 3H₂O(l) which one is true:

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

Enthalpy  of $C{H}_4$ $+$ $\frac{1}{2}{O}_2$ $\to$ $C{H}_{3}OH$ is negative. If the enthalpy of combustion of $C{H}_4$ $and$ $C{H}_{3}OH$ are x and y respectively, then which relation is correct:

For the reaction:

\(C_{3} H_{8} \left(\right. g \left.\right) + 5 O_{2} \left(\right. g \left.\right) \rightarrow 3 CO_{2} \left(\right. g \left.\right) + 4 H_{2} O \left(\right. l \left.\right)\) at constant temperature, ∆H – ∆E is: