1.0 mol of a monoatomic ideal gas is expanded from state (1) to state (2) as shown in the graph below:

   

The work done for the expansion of gas from state (1) to state (2) at 298 K will be:

1. 1617.6 J

2. -1617.6 J

3. 1717.6 J

4. -1717.6 J

The incorrect statement(s) among the following statements is/are -

1. (i), (iv)
2. (ii), (iv)
3. (iii), (iv)
4. (i), (iii)

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)

An enthalpy diagram for a particular reaction is given below:

Which of the following statements is correct?

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-

$\mathrm{}$Consider the given reaction"
\(2 Zn(s) + O_2 (g) \rightarrow 2ZnO(s)\)
For this reaction, \(\Delta H = -693.8~ \text {kJ mol}^{-1}\).
The correct statements among the following are :

1. a and b
2. b and c
3. c and d
4. a and c