For the decomposition of HI at 1000 K (2HI arrow H 2+ I 2 ), the following data were obtained [HI] (M) Rate of decomposition of HI (mol L -1 s -1 ) 0.1 2.75× 10-8 0.2 11 × 10-8 0.3 24.75 × 10-8 The order of reaction is:

Question

For the decomposition of HI at 1000 K (2HI arrow H 2+ I 2 ), the following data were obtained [HI] (M) Rate of decomposition of HI (mol L -1 s -1 ) 0.1 2.75× 10-8 0.2 11 × 10-8 0.3 24.75 × 10-8 The order of reaction is: (A) 1 (B) 2 (C) 0 (D) 1.5

Tardigrade Admin · Accepted Answer

Rate =k[ HI ]n 11 × 10-8=k[0.2]n (1) 2.75 × 10-8=k[0.1]n (2) Dividing eq. (i) by eq. (ii), 4=2n, n=2

Q. For the decomposition of $H I$ at $1000 K$ ( $2 H I \to H_{2} + I_{2}$ ), the following data were obtained
$[H I] (M)$ Rate of decomposition of $H I (m o l L^{- 1} s^{- 1}$ )
$0.1 2.75 \times 1 0^{- 8}$
$0.2 11 \times 1 0^{- 8}$
$0.3 24.75 \times 1 0^{- 8}$
The order of reaction is:

1

2

0

1.5

Rate $= k [H I]^{n}$

$11 \times 1 0^{- 8} = k [0.2]^{n} (1)$

$2.75 \times 1 0^{- 8} = k [0.1]^{n} (2)$

Dividing eq. (i) by eq. (ii),

$4 = 2^{n}, n = 2$

Q. For the decomposition of HI at 1000K (2HI→H2​+I2​ ), the following data were obtained [HI](M) Rate of decomposition of HI(molL−1s−1 ) 0.12.75×10−8 0.211×10−8 0.324.75×10−8 The order of reaction is:

1

2

0

1.5

Rate =k[HI]n 11×10−8=k[0.2]n(1) 2.75×10−8=k[0.1]n(2) Dividing eq. (i) by eq. (ii), 4=2n,n=2

Q. For the decomposition of $H I$ at $1000 K$ ( $2 H I \to H_{2} + I_{2}$ ), the following data were obtained
$[H I] (M)$ Rate of decomposition of $H I (m o l L^{- 1} s^{- 1}$ )
$0.1 2.75 \times 1 0^{- 8}$
$0.2 11 \times 1 0^{- 8}$
$0.3 24.75 \times 1 0^{- 8}$
The order of reaction is:

Rate $= k [H I]^{n}$

$11 \times 1 0^{- 8} = k [0.2]^{n} (1)$

$2.75 \times 1 0^{- 8} = k [0.1]^{n} (2)$

Dividing eq. (i) by eq. (ii),

$4 = 2^{n}, n = 2$