Which of the following statements are 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 statements is true for a reaction where all the reactants and products are in the liquid phase?

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

The enthalpy of \(CH_4 + \dfrac{1}{2 }O_2 \rightarrow\ CH_3OH\)$$ is negative. If enthalpy of combustion of methane and  \(CH_3OH\) are x and y, respectively, then which of the following relations is correct?

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