The reaction $2 N O (g) + C l_{2} (g) \to 2 N O C l (g)$ is second order in $N O$ and first order in $C l_{2}$ . In a volume of $2 d m^{3} . 5$ mole of nitric oxide and $2 m o l$ of $C l_{2}$ were brought together, and the initial rate was $2.4 \times 10^{3} m o l e d m^{- 3} s^{- 1}$ . What will be the rate when half of the chlorine has reacted?

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Solution

$2 N O + C l_{2} \to 2 N O C l$
$- \frac{d R}{d t} = K [N O]^{2} [C l_{2}]$
at $t = 0$ initially
$[N O] = \frac{5}{2} = 2.5 m o l d m^{- 3}$
$[C l_{2}] = \frac{2}{2} = 1 m o l d m^{- 3}$
$- \frac{d R}{d t} = k (2.5)^{2} (1) = 6.25 k$
when flay of $C l_{2}$ reacted then
$[C l_{2}] = \frac{2 - 1}{2} = 0.5 m o l d m^{- 3}$
$[N O] = \frac{5 - 1}{2} = 2 m o l d m^{- 3}$
$- \frac{d R}{d t} = K (2)^{2} \times 0.5$
$= 2 K$

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Similar questions

Q. For the reaction:

2 N O (g) + C l_{2} (g) \to 2 N O C l (g)

, the mixture containing an equimolar mixture of

N O

and

C l_{2}

gases at 0.15

a t m

was half consumed in 175 s. Another experiment, having an initial pressure of 0.35 atm, the mixture was half consumed in 75 s. Find the order of reaction.

Q. For a reaction

2 N O (g) + C l_{2} (g) \to 2 N O C l (g)

, when concentration of

C l_{2}

is doubled the rate of reaction becomes two-times of the original. When the concentration of

N O

is doubled the rate becomes four times. What is the order of the reaction?

Experiment No.	Initial $[N O] (M)$	Initial $[C l_{2}] (M)$	Initial rate of disappearance of $C l_{2} (M / m i n)$
1	0.15	0.15	0.60
2	0.15	0.30	1.20
3	0.30	0.15	2.40
4	0.25	0.25	?

For the reaction,

2 N O_{(g)} + C l_{2 (g)} \to 2 N O C l_{(g)}

The following data were collected. All the measurements were taken at

263 K

(a) Write the expression for rate law.
(b) Calculate the value of rate constant and specify its units.
(c) What is the initial rate of disappearance of $C l$ , in experiment no. 4?

2 N O (g) + C l_{2} (g) \to 2 N O C l (g)

The following data were collected. All the measuremnets were taken at 263 K.

Experiment No.	Initial [NO] (M)	Initial $[C_{2}]$ (M)	Initial rate of disappearance of $C l_{2}$ (M/min)
1	0.15	0.15	0.60
2	0.15	0.30	1.20
3	0.30	0.15	2.40
4	0.25	0.25	?

(a) Write the expression for rate law.
(b) Calculate the value of rate constant and specify its units.
(c) What is the initial rate of disappearance of

C l_{2}

in exp. 4?

Q. The experimental data for the reaction

2 N O (g) + C l_{2} (g) \to 2 N O C l (g)

are given below:

Expt	$[C l_{2}]$	[NO]	Initial rate
1	0.020	0.010	$2.4 \times 10^{- 4}$
2	0.020	0.030	$2.16 \times 10^{- 3}$
3	0.040	0.030	$4.32 \times 10^{- 3}$

The order of the reaction is:

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The reaction 2NO(g)+Cl2(g)→2NOCl(g) is second order in NO and first order in Cl2. In a volume of 2 dm3.5 mole of nitric oxide and 2 mol of Cl2 were brought together, and the initial rate was 2.4×103mole dm−3s−1. What will be the rate when half of the chlorine has reacted?

2NO+Cl2→2NOCl−dRdt=K[NO]2[Cl2]at t=0 initially[NO]=52=2.5moldm−3[Cl2]=22=1moldm−3−dRdt=k(2.5)2(1)=6.25kwhen flay of Cl2 reacted then[Cl2]=2−12=0.5moldm−3[NO]=5−12=2moldm−3−dRdt=K(2)2×0.5=2K