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question_answer1) A drop of solution (volume 0.05 ml) contains \[3.0\times {{10}^{-6}}mole\] of \[{{H}^{+}}\] . If the rate constant of disappearance of \[{{H}^{+}}\] is \[1.0\times {{10}^{7}}mole\] \[litr{{e}^{-1}}\,{{\sec }^{-1}}\] . How long would it take for \[{{H}^{+}}\] in drop to disappear? Give your answer as \[x\times {{10}^{-9}}\] where x is -
question_answer2) The specific rate constant of the decomposition of \[{{N}_{2}}{{O}_{5}}\] is \[0.008{{\min }^{-1}}\] . The volume of \[{{O}_{2}}\] collected after 20 minutes is 16 ml. Find the volume that would be collected at the end of reaction. \[N{{O}_{2}}\] formed is dissolved in \[CC{{l}_{4}}\].
question_answer3) The reaction \[As{{H}_{3}}\left( g \right)\to As\left( s \right)+3/2\,{{H}_{2}}\left( g \right)\] was followed at constant volume at \[310{}^\circ C\] by measuring the gas pressure at intervals. Show from the following figures that reaction is of first order. Time (in hrs) 0 5 7.5 10 Total pressure (in mm) 758 827 856 882
question_answer4) A certain substance A is mixed with an equimolar quantity of substance B. AT the end of an hour A is 75% reacted. Calculate the time when A is 10% unreacted. (Given: order of reaction is Zero).
question_answer5) Two substance \[A\left( {{t}_{1/2}}=5\min s \right)\] and \[B\left( {{t}_{1/2}}=15\min s \right)\] follow first order kinetics are taken in such a ways that initially \[\left[ A \right]=4\left[ B \right]\]. Calculate the time after which the concentration of both the substance will be equal.
question_answer6) Under the same reaction conditions, initial concentration of \[1.386mol/d{{m}^{3}}\] of a substance becomes half in 40 seconds and 20 seconds through first order and zero order kinetics, respectively. Ratio \[\left( \frac{{{k}_{1}}}{{{k}_{0}}} \right)\] of the rate constant for first order \[\left( {{k}_{1}} \right)\] and zero order \[\left( {{k}_{0}} \right)\] of the reaction is -
question_answer7) The rate of a first order reaction is 0.04 mol \[litr{{e}^{-1}}{{s}^{-1}}\] at 10 minutes and 0.03 mol \[litr{{e}^{-1}}{{\sec }^{-1}}\] at 20 minutes after initiation. Find the half life of the reaction.
question_answer8) \[A+B\to \Pr oduct\] For the above reaction following initial rates were given at various initial concentration Initial conc. of A \[M{{L}^{-1}}\] Initial conc. of B in \[M{{L}^{-1}}\] Rate in \[M{{L}^{-1}}{{S}^{-1}}\] 0.1 0.1 0.05 0.2 0.1 0.1 0.1 0.2 0.05 Determine the rate constant.
question_answer9) The concentration of R in the reaction \[R\to P\] was measured as a function of time and the following data is obtained : [R] (molar) 1.0 0.75 0.40 0.10 t (min.) 0.0 0.05 0.12 0.18 The order of the reaction is
question_answer10) An organic compound undergoes first - order decomposition. The time taken for its decomposition to 1/8 and 1/10 of its initial concentration are \[{{t}_{1/8}}\] and \[{{t}_{1/10}}\] respectively. What is the value of \[\frac{\left[ {{t}_{1/8}} \right]}{\left[ {{t}_{1/10}} \right]}\times 10\] ? \[\left( take{{\log }_{10}}2=0.3 \right)\]
question_answer11) The gaseous decompostion reaction, \[A\left( g \right)\to 2B\left( g \right)+C\left( g \right)\] is observed to first order over the excess of liquid water at \[25{}^\circ C\] . It is found that after 10 minutes the total pressure of system is 188 torr and after very long time it is 388 torr. The rate constant of the reaction \[(in~h{{r}^{-1}})\] is: [Given: vapour pressure of \[{{H}_{2}}O\] at \[25{}^\circ \] is 28 torr (In 2=0.7, in 3=1.1, in 10=2.3)]
question_answer12) For the irreversible unimolecular type reaction \[A\xrightarrow{k}\] products in a batch reactor, 80% reactant \[A\left( {{C}_{A0}}=1mole/lit. \right)\] is converted in a 480 second run and conversion is 90% after 18 minute. The order of this reaction is-
question_answer13) The gas phase decomposition \[2{{N}_{2}}{{O}_{5}}\to 4N{{O}_{2}}+{{O}_{2}}\] follows the first order rate law. \[K=7.5\times {{10}^{-3}}{{\sec }^{-1}}\]. The initial pressure of \[{{N}_{2}}{{O}_{5}}\] is 0.1 atm. The time of decomposition of \[{{N}_{2}}{{O}_{5}}\] so that the total pressure becomes 0.15 atm will be
question_answer14) Sucrose decompose in acid solution into glucose and fructose according to a first order rate law, with a half life of 3.33 hour at \[25{}^\circ C\] . what fraction of a sample of sucrose remains after 9.00 hour.
question_answer15) The following data were obtained for the saponification of ethyl acetate using equal concentration of ester alkali. Time (min.) 0 4 10 20 Vol. of acid used (ml.) 8.04 5.3 3.5 2.22 Show that the reaction is of second order.
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