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241. Ammonia and oxygen react at high temperatures according to the equation
4NH₃(g) + 5O₂(g) 4NO(g) → + 6H₂O(g)
In an experiment, the rate of formation of NO was found to be 3.2 x 10^–3 mol L^–1 S^–1. Calculate the rate of disappearance of ammonia and the rate of formation of water.

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242. 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?

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243. For a reaction 2I^– + 2H⁺ → I₂ (s) + H₂(g), if the initial concentration of I^–1 was 0.80 mol L^–1 and concentration after 20 minutes was 0.68 mol L^–1. Calculate the rate of disappearance of I^– and rate of appearance of I₂.

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Long Answer Type

244. The rate of change in concentration of C in the reaction 2A + B → 2C + 3D was reported 1.0 M sec^–1. Calculate the reaction rate as well as rate of change of concentration of A, B and D.

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Short Answer Type

245. For the reaction: 3H₂(g) + N₂ (g) → 2NH₃(g) express the rate of reaction in terms of

- \frac{d [H_{2}]}{dt}, \frac{- d [N_{2}]}{dt} and \frac{d [{NH}_{3}]}{dt} .

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246. How is the rate of formation of NO₂ related to the rate of disappearance of NO and O₂ in the reaction given below:
$2 NO (g) + O_{2} (g) \to 2 {NO}_{2} (g)$

Formation of NO₂ rate of disappearnace of NO and O₂ is given by rate equation:

Rate = \frac{1}{2} \frac{d [{NO}_{2}]}{dt} = \frac{- 1}{2} \frac{d [NO]}{dt} = \frac{- d [O_{2}]}{dt}

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247. How is the rate of formation of Br₂ is related to the rate of disappearance of Br, BrO₃^– and H⁺ in the reaction given below:

5 Br - (aq) + {BrO}_{3}^{-} (aq) + 6 H^{+} (aq) \to 3 {Br}_{2} (aq) + 3 H_{2} O (l)

123 Views

248. The gas phase decomposition of acetaldehyde
CH₃CHO(g) → CH₄(g) + CO(g)
at 680 K is observed to follow the rate expression

rate = \frac{- d [{CH}_{3} CHO]}{dt} = k {[{CH}_{3} CHO]}^{1 / 2}

If the rate of the decomposition is followed by monitoring the partial pressure of the acetaldehyde, we can express the rate as

\frac{{dp}_{{CH}_{3} CHO}}{dt} = k {[p_{{CH}_{3} CHO}]}^{3 / 2}

If the pressure is measured in atmosphere and time in minutes then
(i) What are the units of the rate of reaction?
(ii) What are the units of rate constant k?

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249. State the order with respect to each reactant and overall order for the reaction
2H₂(g) + 2NO(g) → 2H₂O(g) + N₂(g)
Rate = k[H₂][NO]²

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250. For a reaction: A + B → Products
The rate law expression is, rate = k[A]^1/3.[B]². What is the order of reaction?

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246. How is the rate of formation of NO2 related to the rate of disappearance of NO and O2 in the reaction given below: 2NO(g) + O2(g) → 2NO2(g)

246. How is the rate of formation of NO₂ related to the rate of disappearance of NO and O₂ in the reaction given below:
$2 NO (g) + O_{2} (g) \to 2 {NO}_{2} (g)$