{"id":35308,"date":"2022-09-09T09:41:34","date_gmt":"2022-09-09T04:11:34","guid":{"rendered":"https:\/\/apboardsolutions.guru\/?p=35308"},"modified":"2022-09-09T09:41:34","modified_gmt":"2022-09-09T04:11:34","slug":"ap-inter-2nd-year-chemistry-study-material-chapter-3b","status":"publish","type":"post","link":"https:\/\/apboardsolutions.guru\/ap-inter-2nd-year-chemistry-study-material-chapter-3b\/","title":{"rendered":"AP Inter 2nd Year Chemistry Study Material Chapter 3(b) Chemical Kinetics"},"content":{"rendered":"

Andhra Pradesh BIEAP AP Inter 2nd Year Chemistry Study Material<\/a> Lesson 3(b) Chemical Kinetics Textbook Questions and Answers.<\/p>\n

AP Inter 2nd Year Chemistry Study Material Lesson 3(b) Chemical Kinetics<\/h2>\n

Very Short Answer Questions<\/span><\/p>\n

Question 1.
\nDefine the speed or rate of a reaction.
\nAnswer:
\nThe change in the concentration of a reactant (or) product in unit time is called the speed or rate of a reaction.
\n(or)
\nThe decrease in the concentration of a reactant (or) increases in the concentration of product per unit time.<\/p>\n

Question 2.
\nAssuming that the volume of the system is constant, derive the expression for the average rate of the system R \u2192 P in terms of R and R [time = ‘t’ sec] [R = reactant, P = product].
\nAnswer:
\n\"AP<\/p>\n

\"AP<\/p>\n

Question 3.
\nWhat are the units of rate of reaction ?
\nAnswer:
\nUnits of rate of reaction – moles\/Lit \u00d7 sec – moles. Lit-1<\/sup> . sec-1<\/sup><\/p>\n

Question 4.
\nDraw the graphs that relate the concentrations .(C) of the reactants and the reaction times (t) and the concentrations of the products (C) and the reaction times (t) in chemical reactions.
\nAnswer:
\n\"AP<\/p>\n

Question 5.
\nWrite the equation for the rate of the reaction.
\n\\(5 \\mathrm{Br}_{(\\mathrm{aq})}^{-}+\\mathrm{BrO}_{3(\\mathrm{aq})}^{-}+6 \\mathrm{H}_{(\\mathrm{aq})}^{+} \\longrightarrow 3 \\mathrm{Br}_{2(\\mathrm{aq})}+3 \\mathrm{H}_2 \\mathrm{O}_{(\\text {) }}\\)
\nAnswer:
\nGiven reaction is
\n\\(5 \\mathrm{Br}_{(\\mathrm{aq})}^{-}+\\mathrm{BrO}_{3(\\mathrm{aq})}^{-}+6 \\mathrm{H}_{(\\mathrm{aq})}^{+} \\longrightarrow 3 \\mathrm{Br}_{2(\\mathrm{aq})}+3 \\mathrm{H}_2 \\mathrm{O}_{(\\text {) }}\\)
\nRate of reaction = \\(=-\\frac{1}{5} \\frac{\\Delta\\left[\\mathrm{Br}^{-}\\right]}{\\Delta \\mathrm{t}}=\\frac{-\\Delta\\left[\\mathrm{BrO}_3^{-}\\right]}{\\Delta \\mathrm{t}}=\\frac{-1}{6} \\frac{\\Delta\\left[\\mathrm{H}^{+}\\right]}{\\Delta \\mathrm{t}}=\\frac{-1}{3} \\frac{\\Delta\\left[\\mathrm{Br}_2\\right]}{\\Delta \\mathrm{t}}=\\frac{1}{3} \\frac{\\Delta\\left[\\mathrm{H}_2 \\mathrm{O}\\right]}{\\Delta \\mathrm{t}}\\)<\/p>\n

Question 6.
\nWhat is rate law ? Illustrate with an example.
\nAnswer:
\nThe equation that describes mathematically the dependence of the rate of a reaction on the concentration terms of the reactions is known as the rate equation (or) rate law.
\nEg : 2A + 3B \u2192 3C
\nRate, of the given reaction \u221d [A]2<\/sup> [B]3<\/sup><\/p>\n

\"AP<\/p>\n

Question 7.
\nMention a reaction for which the exponents of concentration terms are not the same as their stoichiometric coefficients in the rate equation.
\nAnswer:
\nThe following are the reactions for which the exponents of concentration terms are not the same as their stoichiometric coefficients in the rate equation.
\nCHCl3<\/sub> + Cl2<\/sub> \u2192 CCl4<\/sub> + HCl
\nrate = k[CHCl3<\/sub>] [Cl2<\/sub>]1\/2<\/sup>
\nCH3<\/sub>COOC2<\/sub>H5<\/sub> + H2<\/sub>O \u2192 CH3<\/sub>COOH + C2<\/sub>H5<\/sub>OH
\nrate = k[CHCOOC2<\/sub>H5<\/sub>] [H2<\/sub>O]1\/2<\/sup><\/p>\n

Question 8.
\nDefine Order of a reaction. Illustrate your answer with an example. [T.S. Mar. 15]
\nAnswer:
\nOrder of a reaction : The sum of the powers of the concentration terms of the reactants present in the rate equation is called order of a reaction.
\nOrder of a reaction can be 0, 1, 2, 3, and even a fraction
\nEg. : 1) N2<\/sub>O5<\/sub> \u2192 N2<\/sub>O4<\/sub> + \\(\\frac{1}{2}\\) O2<\/sub>
\nrate \u221d [N2<\/sub>O5<\/sub>]
\n\u2234 It is a first order reaction.<\/p>\n

2) 2N2<\/sub>O \u2192 2N2<\/sub> + O2<\/sub>
\nrate \u221d [N2<\/sub>O]2<\/sup>
\n\u2234 It is 2nd<\/sup> order reaction.<\/p>\n

Question 9.
\nWhat are elementary reactions ?
\nAnswer:
\nThe reactions taking place in one step are called elementary reactions.<\/p>\n

Question 10.
\nWhat are complex reactions ? Name one Complex reaction.
\nAnswer:
\nA sequence of elementary reactions, reactants give the products, the reactions are called complex reactions.
\nEg: Oxidation of Ethane to CO2<\/sub> and H2<\/sub>O passes through a series of intermediate steps in which alcohol, aldehyde and acid are formed.<\/p>\n

\"AP<\/p>\n

Question 11.
\nGive the units of rate constants for Zero, first order and second order reactions.
\nAnswer:
\n\"AP<\/p>\n

Question 12.
\nDefine molecularity of a reaction. Illustrate with an example.
\nAnswer:
\nThe number of reacting species (atoms, ions or molecules) taking parts in an elementary reaction, which must colloid simultaneously to bring about a chemical reaction is called molecularity of a reaction.
\nNH4<\/sub>NO2<\/sub> \u2192 N2<\/sub> + 2H2<\/sub>O (Unimolecular)
\n2HI \u2192 H2<\/sub> + I2<\/sub> (Bimolecular)
\n2NO + O2<\/sub> \u2192 2NO2<\/sub> (Trimolecular)<\/p>\n

Question 13.
\nWhat is rate determining step in a complex reaction ?
\nAnswer:
\nThe overall rate of a reaction is controlled by the slowest step in a reaction is called the rate determining step in a complex reaction.<\/p>\n

Question 14.
\nGive the mechanism for the decomposition reaction of H2<\/sub>O2<\/sub> in alkaline medium catalysed by I–<\/sup> ions.
\nAnswer:
\nChemical equation of decomposition of H2<\/sub>O2<\/sub> in alkaline medium is
\n\"AP
\nMechanism:<\/p>\n