The given data are for the reaction 2 N O ( g ) + C l ( g ) → 2 N O C l ( g ) at 298 K [ C l 2 ] [NO] Initial rate (mol L - 1 s e c - 1 ) I 0.05 M 0.05 M 1 × 1 0 - 3 I I 0.15 M 0.05 M 3 × 1 0 - 3 I I I 0.05 M 0.15 M 9 × 1 0 - 3 The rate law of the reaction is

Question

The given data are for the reaction 2 N O ( g ) + C l ( g ) → 2 N O C l ( g ) at 298 K [ C l 2 ] [NO] Initial rate (mol L - 1 s e c - 1 ) I 0.05 M 0.05 M 1 × 1 0 - 3 I I 0.15 M 0.05 M 3 × 1 0 - 3 I I I 0.05 M 0.15 M 9 × 1 0 - 3 The rate law of the reaction is, rate = k [ N O ] [ C l 2 ], rate = k [ C l 2 ] [ N O ] 2, rate = k [ C l 2 ] 2 [ N O ], rate = k [ C l 2 ]

MARKS App · Accepted Answer

1 × 1 0 - 3 = k [ 0.05 ] α [ 0.05 ] β …(i) 3 × 1 0 - 3 = k [ 0.15 ] α [ 0.05 ] β …(ii) 9 × 1 0 - 3 = k [ 0.05 ] α [ 0.15 ] β …(iii) From (i) and (ii), α = 1 and from (i) and (iii), β = 2 So rate = k [ N O ] 2 [ C l 2 ] 1 .

	$[C l_{2}]$	[NO]	Initial rate (mol $L^{- 1} s e c^{- 1}$ )
$I$	0.05 M	0.05 M	$1 \times 1 0^{- 3}$
$I I$	0.15 M	0.05 M	$3 \times 1 0^{- 3}$
$I I I$	0.05 M	0.15 M	$9 \times 1 0^{- 3}$

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