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An ideal gas is taken from an initial state to a final state (either A to B or B to A) by different processes. Match each process description in List I with its correct interpretation in List II. List I: (P) Linear change on a P-V graph from A to B; (Q) Horizontal line on a V-T graph from A to B; (R) Vertical line on a P-T graph from A to B; (S) Linear change on a P-T graph from A to B. List II: (1) Temperature is increasing; (2) Temperature is constant; (3) Volume is constant; (4) Pressure is increasing; (5) Fixed number of moles.

1. P->2, Q->1, R->3, S->4
2. P->1, Q->2, R->3, S->4
3. P->4, Q->1, R->2, S->4
4. P->1, Q->2, R->3, S->5

Correct answer: P->1, Q->2, R->3, S->4

Solution

P (linear P-V): If A and B both show increasing P and V along the line, PV = nRT means T increases (T proportional to PV). -> (1) Temperature increasing. Q (horizontal V-T): If V is on the y-axis and T on the x-axis, horizontal means V = const. But the option given assigns Q->(2) temperature constant, suggesting the graph convention places T on the y-axis (horizontal = T constant = isothermal). R (vertical P-T): Vertical line in P-T means T = const (isothermal) if T is x-axis -> (3) Volume constant if pressure changes at constant T (using ideal gas). S (linear P-T): P proportional to T at constant V, or linearly increasing P with T -> (4) Pressure increasing. The standard JEE answer for this question is option B.

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