A system that can neither exchange matter nor energy with the surroundings is classified as:

1. Open system

2. Isolated system

3. Closed system

4. Both (1) & (2)

The enthalpy change for the reaction is called

         $C_2{H}_4+3O_2\to 2C{O}_2+2H_{2}O$

1. Enthalpy of formation

2. Enthalpy of vaporisation

3. Enthalpy of sublimation

4. Enthalpy of combustion

Calculate the amount of heat required to raise the temperature of 12.0 g of iron from 25°C to 100°C.
[Given: specific heat of iron is 0.45 J ^∘C^-1 g^-1 ]

1. 0.945 kJ

2. 0.405 kJ

3. 0.285 kJ

4. 12.34 kJ

In which of the following process, entropy change (∆S) is negative?

1. Hg(l) → Hg(g)

2. C_graphite → C_diamond

3. AgNO₃(s) → AgNO₃(aq)

4. l₂(s) \(\xrightarrow[]{\Delta }\) l₂₍g)

Which of the following are not state functions?

I. q + w

II. q 

III. w

IV. H - TS

1. I, II & III

2. II & III

3. I & IV

4. II, III & IV

The enthalpy and entropy change for the reaction :

Br₂(l)+Cl₂(g) $\to$ 2BrCl(g) are 30 kJ mol^-1 and 105 JK^-1 mol^-1 respectively.

The temperature at which the reaction will be in equilibrium is :

1. 285.7 K

2. 273 K

3. 450 K

4. 300 K

Which one of the following reactions obeys  ∆H ≠ ∆E?

The hydrolysis of sucrose is represented by the reaction:

At 300 K, the equilibrium constant (K_c) for the reaction is 2 × 10¹³.

Calculate the standard Gibbs free energy change (ΔᵣG°) for the reaction at this temperature:

1. 8.314 J mol^-1 K^-1$\times$300 K$\times$ln (2$\times$10¹³)

2. 8.314 J mol^-1 K^-1$\times$300 K$\times$ln (3$\times$10¹³)

3. -8.314 J mol^-1 K^-1$\times$300 K$\times$ln (4$\times$10¹³)

4. -8.314 J mol^-1 K^-1$\times$300 K$\times$ln (2$\times$10¹³)

Nitrogen gas (N₂) is confined in a cylinder fitted with a movable piston and undergoes an adiabatic expansion.
Which of the following statements is correct for this process?

1. q=w

2. ∆U=w

3. ∆U=0

4. ∆U=q

Match the terms in List I with their corresponding descriptions in List II:

Codes: