Book Store

Download books and chapters from book store.
Currently only available for.
CBSE Gujarat Board Haryana Board

Previous Year Papers

Download the PDF Question Papers Free for off line practice and view the Solutions online.
Currently only available for.
Class 10 Class 12

Chemical Kinetics

Nitrogen dioxide (NO₂) reacts with fluorine (F₂) to form nitryl fluoride (NO_zF) according to the reaction

2 {NO}_{2} (g) + F_{2} (g) \to 2 {NO}_{2} F (g)

Write the instantaneous rate of reaction in terms of
(i) rate of formation of NO₂ ,F
(ii) rate of disappearance of NO₂(iii) rate of disappearance of F₂.

Nitrogen dioxide (NO₂) reacts with fluorine (F₂) to form nitryl fluoride (NO_zF) according to the reaction

$2 {NO}_{2} (g) + F_{2} (g) \to 2 {NO}_{2} F (g)$

(i) Rate of formation of ${NO}_{2} F (r) = \frac{d ({NO}_{2} F)}{dt} .$
(ii) Rate of disappearance of ${NO}_{2} (r) = - \frac{d ({NO}_{2})}{dt} .$
(iii) Rate of disappearance of $F_{2} (r) = - \frac{d (F_{2})}{dt} .$

435 Views

The pressure of a gas decomposing at the surface of a solid catalyst has been measured at different times and the results are given below:

t/s	0	100	200	300
p/pascal	4.0 x 10³	3.5 x 10³	3.0 x 10³	2.5 x 10³

Determine the order of reaction, its rate constant and half-life period.

The rate of reaction between different time interval is

As rate remains constant, therefore, reaction is of zero order.

121 Views

The decomposition of N₂O₅ in CCl₄ at 318 K has been studied by monitoring the concentration of N₂O₅ in the solution. Initially the concentration of N₂O₅ is 2.33 M and after 184 minutes, it is reduced to 2.08 M. The reaction takes place according to the equation:

2 N_{2} O_{5} (g) \to 4 {NO}_{2} (g) + O_{2} (g)

Calculate the average rate of this reaction in terms of hours, minutes and seconds. What is the rate of production of NO₂ during this period?

\frac{1}{2} [- ∆ [N_{2} O_{5}] / ∆ (t)] = - \frac{1}{2} [2.08 - 2.33] M / 184 \min

= 6.79 \times 10^{- 4} M / \min = 6.79 \times 10^{- 4} M / \min \times 60 \min / 1 hr . = 4.07 \times 10^{- 2} M / hr = 6.79 \times 10^{- 4} M \times 1 \min / 60 s = 1.13 \times 10^{- 5} M / s

Again,

Rate = \frac{1}{4} d [{NO}_{2}] / dt

d [{NO}_{2}] / dt = 6.79 \times 10^{- 4} \times 4 {ML}^{- 1} / \min = 2.72 \times 10^{- 3} {ML}^{- 1} / \min

1240 Views

A first order reaction has a specific reaction rate of 10^–3. How much time will it take for 10 g of the reactant to reduce to 2.5 g. Given log 2 = 0.301, log 4 = 0.6021, log 6 = 0.778.

For a first order reaction

t = \frac{2.303}{k} \log \frac{a}{a - x}

Here initial concentration, a = 10 g and concentration left after time t sec = 2.5 g i.e., 2.5 g i.e., (a – x) = 2.5 g.
Specific reaction constant k = 10^–3 sec^–1.
∴ Time required for the reactant to reduce to

= \frac{2.303}{10^{- 3}} \times \log \frac{10}{2.5} = \frac{2.303}{10^{- 3}} \log 4 = \frac{2.303}{10^{- 3}} \times 0.6021 = 1386.6 \sec .

724 Views

In the Arrhenius equation for a certain reaction, the value of A and Ea (activation energy) are 4 x 10¹³ sec^–1 and 98.6 mol^–1 respectively, If the reaction is of first order, at what temperature will its half life period be the minutes?

By using the half life reaction equation

k = \frac{0.693}{t_{1 / 2}} = \frac{0.693}{10 \times 60} = 1.155 \times 10^{- 3}

According to Arrhenius equation

\log k = \log A - \frac{Ea}{2.303 RT}

\log 1.155 \times 10^{- 3} = \log 4 \times 10^{13} - \frac{98.6}{2.303 \times 8.314 \times T} or T = 311.65 K

149 Views

Chapter Chosen

Book Chosen

Subject Chosen

Book Store

Previous Year Papers

Chemical Kinetics

In the Arrhenius equation for a certain reaction, the value of A and Ea (activation energy) are 4 x 10¹³ sec^–1 and 98.6 mol^–1 respectively, If the reaction is of first order, at what temperature will its half life period be the minutes?

Chapter Chosen

Book Chosen

Subject Chosen

Book Store

Previous Year Papers

Chemical Kinetics

In the Arrhenius equation for a certain reaction, the value of A and Ea (activation energy) are 4 x 1013 sec–1 and 98.6 mol–1 respectively, If the reaction is of first order, at what temperature will its half life period be the minutes?

In the Arrhenius equation for a certain reaction, the value of A and Ea (activation energy) are 4 x 10¹³ sec^–1 and 98.6 mol^–1 respectively, If the reaction is of first order, at what temperature will its half life period be the minutes?