In the reaction BrO^-₃ (aq) + 5 Br ^- (aq) + 6 H⁺ \(\longrightarrow\) 3 Br₂(I) + 3 H₂O (l), the rate of apperance of bromine (BHr₂) is related to the disapearance of bromide uions as follows :

 The rate of  the reaction 2 NO + CI₂ \(\rightarrow\) 2NOCI is given by the rate equation : rate = k [NO]₂ [CI₂]. The value  of the rate constant can be increased by

The molecularity and order of the reaction 2 NO (g) + O₂ (g) \(\rightarrow\)2NO₂ (g) are respectively

Consider the reaction : CI₂ (aq) + H₂S (aq) \(\rightarrow\) S (s) + 2 H⁺ (aq) +2 CI^- (aq) The rate equation for this reaction is rate k [CI₂] [H₂S] Which of these mechanisms is / are consistant with this rate equation ?
A. CI₂+H₂S \(\longrightarrow\) H⁺ + CI- + CI⁺ HS^- (slow) ; CI+ Hs^-  \(\longrightarrow\) H⁺ + CI^- + S (fast)
B. H₂S \(\rightleftharpoons \) H⁺ + HS - (fast equilibrium) ; CI₂ + HS^-  \(\longrightarrow\) 2 CI^- + H⁺ S (slow)

For the reaction R \(\longrightarrow\) P, a graph of [R] against time is found to be a straight line with negative slope. What is the order of reaction ?

How does the value of rate constant vary with reactant concentration?

A substance with initial concentration 'a' follows zero order kine ics with the rate constant 'k' mol L^-1s^-1.  In how much time will the reaction go to completion?

When is the rate of reaction equal to specific reaction rate?

According to Arrhenius, rate of reaction increases with increase in temperature. Give reasons.

For a gaseous reaction, the units of the reaction are..............

In the plot of concentratiuon of reactant versus time, the tangent at any instant of time has a......... slope (opositive or negative or zero).

If the rate of reaction, 4 NH₃ + O₂ \(\longrightarrow\) 2 NO + 5 H₂O at any instant of time is 9 \(\times\) 10^-4 mol L^-1 s^-1, then rate of disapperance of NH₃ is ......... .

The rate of reaction when the concentration of each reactant is taken as unity is called ......... .

In the reaction, 2 NO₂ (g)  + F₂ (g) \(\longrightarrow\) 2 NO₂ F (g) , order with respect to NO₂ is................ and that with respect to F₂ is ............ . 

The reaction between H₂(g) and O₂(g) is highly feasible yet allowing the gases to stand at room temperature in the same vessel does not lead to the formation of water.  Explain.

Oxygen is available in plenty in air yet fuels do not burn by themselves at room temperature.  Explain.

Why is the probability of reaction with molecularity higher than three very rare?

Why does the rate of any reaction generally decreases during the course of the reaction?

Thermodynamic feasibility of the reaction alone cannot decide the reaction.  Explain with the help of one example.

In some cases it is found that a large number of colliding molecules have energy more than threshold energy but yet the reaction is slow.  Why?

With the help of diagram explain the role of activated complex in a reaction.

What is physical significance of energy of activation? Explain with diagram.

The thermal decomposition of HCO₂H is a first-order reaction with a rate constant of 2.4 \(\times\) 10^-3 s^-1 at a certain temperature.  Calculate how long will it take for three-fourths of initial quantity of HCO₂H to decompose.  (log 0.25 = - 0.6021)

Explain the terms:
(i) Rate determining step of a reaction
(ii) Molecularity of a reaction

Show that in case of first order reaction, the time required for 99.9% of the reaction to complete is 10 times that required for half of the reaction to take place. [log 2 = 0.301]

At constant temperature and volume, X decomposes as 2 X (g) \(\longrightarrow\)  3 Y (g) + 2 Z (g). P_x is the partial pressure of X.

(i) What is the order of reaction with respect to X?  
(ii) Find the time for 75% completion of the reaction.
(iii) Find the total pressure when pressure of X is 700 mm of Hg.