37.8 g N2O5 was taken in a 1L reaction vessel and allowed to undergo the following reaction at 500 K 2N2O5(g) 2N2O4(g) + O2(g) The total pressure at equilibrium was found to be 18.65 bar. Then, Kp = _

Question

37.8 g N2O5 was taken in a 1L reaction vessel and allowed to undergo the following reaction at 500 K 2N2O5(g) 2N2O4(g) + O2(g) The total pressure at equilibrium was found to be 18.65 bar. Then, Kp = ___________ × 10–2 [nearest integer] Assume N2O5 to behave ideally under these conditions. Given R = 0.082 bar L mol–1 K–1

Prashant Kotian · Accepted Answer

Correct answer: .. ni = 8 . = 0.35 2N2O5(g) 2N2O4(g) + O2(g) ni 0.35 0 0 neq 0.35 – x x x/2 PeqV = neqRT  x = 0.21 Kp = O N O O N ) P ( ) P ( ) P ( 2 4 = 2 . 455 . 24 . 65 . 455 . 105 . 65 . 455 . 21 .                      = 9.62 = 962 × 10–2 | JEE(Main) 2025 | DATE : 24-01-2025 (SHIFT-1) | PAPER-1 | CHEMISTRY PAGE # 8

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