Assertion:  $∆\mathrm{H}$ is positive for endothermic reactions.

Reason: If the total enthalpy of reactants and products are H_r & Hp respectively, then for an endothermic reaction H_R < H_P.

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

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

3. Assertion is a true statement but reason is false.

4. Both assertion and reason are false statements.

Assertion: $C_{diamond}\to C_{graphite}$

$∆H and ∆U are same for this reaction.$

Reason: Entropy increases during the conversion of diamond to graphite.

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

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

3. Assertion is a true statement but reason is false.

4. Both assertion and reason are false statements.

For one mole of an ideal gas, which of these statements must be true?
(I) U and H each depend only on temperature.
(II) Compressibility factor z is not equal to 1.
(III) C_{P, m} – C_{V, m} = R
(IV) dU = C_VdT for any process.
1.  (I), (III) and (IV)
2.  (II), (III) and (IV)
3.  (III) and (IV)
4.  (I) and (III)

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 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