Consider the kinetic data given in the following table for the reaction A + B + C → Product. Experiment No. A m o l   d m - 3 B m o l   d m - 3 C m o l   d m - 3 Rate of reaction m o l   d m - 3 s - 1 1 0.2 0.1 0.1 6.0 × 10 - 5 2 0.2 0.2 0.1 6.0 × 10 - 5 3 0.2 0…

Question

Consider the kinetic data given in the following table for the reaction

A + B + C \to

Product.

Experiment No.	$[A]$ $(m o l {d m}^{- 3})$	$[B]$ $(m o l d m^{- 3})$	$[C]$ $(m o l d m^{- 3})$	Rate of reaction $(m o l d m^{- 3} s^{- 1})$
$1$	$0.2$	$0.1$	$0.1$	$6.0 \times 10^{- 5}$
$2$	$0.2$	$0.2$	$0.1$	$6.0 \times 10^{- 5}$
$3$	$0.2$	$0.1$	$0.2$	$1.2 \times 10^{- 4}$
$4$	$0.3$	$0.1$	$0.1$	$9.0 \times 10^{- 5}$

The rate of the reaction for

[A] = 0.15 m o l d m^{- 3}, [B] = 0.25 m o l d m^{- 3}

and

[C] = 0.15 m o l d m^{- 3}

is found to be

Y \times 10^{- 5} m o l d m^{- 3} s^{- 1} .

The value of

Y

is __________

Aicharya · Accepted Answer

r = k [ A ] a [ B ] b [ C ] c 6 × 10 - 5 = k ( 0.2 ) a ( 0.1 ) b ( 0.1 ) c ..... (1) 6 × 10 - 5 = k ( 0.2 ) a ( 0.2 ) b ( 0.1 ) c ...... (2) 1.2 × 10 - 4 = k ( 0.2 ) a ( 0.1 ) b ( 0.2 ) c ...... (3) 9 × 10 - 5 = k ( 0.3 ) a ( 0.1 ) b ( 0.1 ) c ...... (4) From equation (1) and (ii) : b = 0 From equation (1) and (iii) : c = 1 From equation (1) and (iv) : a = 1 Put x , y and z in equation (i) we get; 6 × 10 - 5 = k ( 0.2 ) 1 ( 0.1 ) 0 ( 0.1 ) 1 r = 3 × 10 - 3 [ A ] [ C ] For [ A ] = 0.15 mol dm - 3 [ B ] = 0.25 mol dm - 3 [ C ] = 0.15 mol dm - 3 r = 3 × 10 - 3 × 0.15 × 0.15 r = 6.75 × 10 - 5 ∴ r = 6.75

Consider the kinetic data given in the following table for the reaction A + B + C → Product.…

Solution

Consider the kinetic data given in the following table for the reaction A + B + C &#8594; Product.…

Solution

Consider the kinetic data given in the following table for the reaction A + B + C → Product.…