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question_answer1) For a chemical reaction, \[2X+Y\xrightarrow{{}}Z\], the rate of appearance of Z is \[0.05\text{ }mol\text{ }{{L}^{-\,1}}\] per min. Find the rate of disappearance of x in \[mol\text{ }{{L}^{-1}}\text{ }mi{{n}^{-1}}\].
question_answer2) For the reaction at 273 K \[NO(g)+{{O}_{3}}(g)\xrightarrow{{}}N{{O}_{2}}(g)+{{O}_{2}}(g)\] It is observed that the pressure of NO(g) falls from 700 mm Hg to 500 mm Hg in 250 s. Calculate the average rate of reaction in \[{{10}^{-\,3}}\text{ }atm\text{ }{{s}^{-\,1}}\].
question_answer3) For a first order reaction, calculate the ratio between the time taken to complete 3/4th of the reaction and time taken to complete half of the reaction.
question_answer4) The half-life period and initial concentration for a reaction areas follows. Initial concentration (M) 350 540 158 \[{{t}_{1/2}}\] (hr) 425 275 941 What is order of reaction?
question_answer5) The rate of a reaction triples when temperature changes from \[20{}^\circ C\] to \[50{}^\circ C\]. Calculate energy of activation for the reaction in \[kJ\text{ }mo{{l}^{-\,1}}\,(R=8.314\text{ }J{{K}^{-\,1}}\,mo{{l}^{-1}}).\]
question_answer6) Sucrose decomposes in acid solution into glucose and fructose according to the first order rate law with \[{{t}_{1/2}}=3.00\] hours. What fraction of the sample of sucrose remains after 8 hours?
question_answer7) A reaction takes place in various steps. The rate constant for first, second, third and fifth steps are \[{{k}_{1}},\,{{k}_{2}},\,{{k}_{3}}\] and \[{{k}_{5}}\] respectively. The overall rate constant is given by \[k=\frac{{{k}_{2}}}{{{k}_{3}}}{{\left( \frac{{{k}_{1}}}{{{k}_{5}}} \right)}^{1/2}}\]. If activation energy are 40, 60, 50 and 10 kJ/mol respectively, find the overall energy of activation (kJ/mol).
question_answer8) The half-life decomposition of gaseous \[C{{H}_{3}}CHO\] at constant temperature but at initial pressure of 3 64 mm and 170 mm of Hg were 410 sec, and 880 sec respectively. Find the order of the reaction.
question_answer9) A gaseous reaction \[{{X}_{2}}(g)\xrightarrow{{}}Y+\frac{1}{2}Z(g)\] There is increase in pressure from 100 mm to 120 mm in 5 minutes. Calculate the rate of disappearance of \[{{X}_{2}}\] in mm\[mi{{n}^{-1}}\].
question_answer10) The reaction \[X\to Y\] is an exothermic reaction. Activation energy of the reaction for X into Y is \[150\text{ }kJ\text{ }mo{{l}^{-1}}\]. Enthalpy of reaction is \[135\text{ }kJ\text{ }mo{{l}^{-1}}\]. Calculate the activation energy for the reverse reaction, \[Y\to X\,\,in\text{ }kJ\text{ }mo{{l}^{-1}}\].
question_answer11) 2 g of a radioactive sample having half-life of 15 days was synthesised on 1st Jan. 2009. What is the amount of the sample left behind on 1st March, 2009 (including both the days) in g?
question_answer12) Half-lives of decomposition of \[N{{H}_{3}}\] on the surface of a catalyst for different initial pressures are given as: P (torr) 200 300 500 \[{{t}_{1/2}}(min)\] 10 15 25 Find the order of the reaction.
question_answer13) The decomposition of ammonia on tungsten surface at 500 K follows zero order kinetics. The half-life period of this reaction is 45 minutes when the initial pressure is 4 bar. Find the half-life period (in minutes) of the reaction when the initial pressure is 16 bar at the same temperature.
question_answer14) In a chemical reaction A is converted into B. The rates of reaction, starting with initial concentrations of A as \[2\times {{10}^{-\,3}}\text{ }M\] and \[1\times {{10}^{-\,3}}\text{ }M\], are equal to \[2.40\times {{10}^{-\,4}}\text{ }M{{s}^{-\,1}}\] and \[0.60\times {{10}^{-\,4}}M{{s}^{-\,1}}\]respectively. Find the order of reaction with respect to reactant A.
question_answer15) The instantaneous rate of disappearance of \[MnO_{4}^{-}\] ion in the following reaction is\[4.56\times {{10}^{-\,3}}\,M{{s}^{-\,1}}\]. \[2MnO_{4}^{-}+10{{I}^{-}}+16{{H}^{+}}\to 2M{{n}^{2+}}+5{{I}_{2}}+\,8{{H}_{2}}O\] Find the rate of appearance \[{{I}_{2}}\,in\,\,M{{s}^{-\,1}}\]
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