{"id":21706,"date":"2020-01-28T12:59:11","date_gmt":"2020-01-28T07:29:11","guid":{"rendered":"https:\/\/kseebsolutions.guru\/?p=21706"},"modified":"2021-07-02T15:26:27","modified_gmt":"2021-07-02T09:56:27","slug":"1st-puc-chemistry-previous-year-question-paper-march-2019-north","status":"publish","type":"post","link":"https:\/\/kseebsolutions.guru\/1st-puc-chemistry-previous-year-question-paper-march-2019-north\/","title":{"rendered":"1st PUC Chemistry Previous Year Question Paper March 2019 (North)"},"content":{"rendered":"

Students can Download 1st PUC Chemistry Previous Year Question Paper March 2019 (North), Karnataka 1st PUC Chemistry Model Question Papers with Answers<\/a> helps you to revise the complete Karnataka State Board Syllabus and score more marks in your examinations.<\/p>\n

Karnataka 1st PUC Chemistry Previous Year Question Paper March 2019 (North)<\/h2>\n

Time: 3.15 Hours
\nMax Marks: 70<\/p>\n

Instruction:<\/p>\n

    \n
  1. \n
      \n
    1. The questions paper has five parts A, B, C, D and E. All parts are compulsory.<\/li>\n
    2. Write balanced chemical equations and draw labeled diagram wherever allowed.<\/li>\n
    3. Use log tables and simple calculations f necessary (use of scientific calculations is not allowed).<\/li>\n<\/ol>\n<\/li>\n<\/ol>\n

      Part – A<\/span><\/p>\n

      I. Answer ALL of the following (each question carries one mark): ( 10 \u00d7 1 = 10 )<\/span><\/p>\n

      Question 1.
      \nWhat is the S.I. unit of Electric Current?
      \nAnswer:
      \nampere (or) A.<\/p>\n

      Question 2.
      \nState Dalton’s law of Partial Pressure.
      \nAnswer:
      \n“The total pressure exerted by a mixture of non-reacting gases is equal to the sum of the partial pressures of all the component gases at constant temperature.”<\/p>\n

      Question 3.
      \nWrite the conjugate base for HCO3<\/sub>–<\/sup>.
      \nAnswer:
      \nCO3<\/sub>-2<\/sup>.<\/p>\n

      \"KSEEB<\/p>\n

      Question 4.
      \nWrite the valence shell electronic configuration of P-block elements.
      \nAnswer:
      \nnS2<\/sup>.p1-6<\/sup>.<\/p>\n

      Question 5.
      \nAssign the oxidation number of ‘Mn’ in MnO–<\/sup>4<\/sub>.
      \nAnswer:
      \n+7.<\/p>\n

      Question 6.
      \nName the alkali metal which has high hydration enthalpy.
      \nAnswer:
      \nLithium.<\/p>\n

      Question 7.
      \nGive the chemical formula of Borax.
      \nAnswer:
      \nNa2<\/sub>B4<\/sub>O7<\/sub> 10H2<\/sub>O.<\/p>\n

      Question 8.
      \nWhat are silicones?
      \nAnswer:
      \nPolymeric organo-silicon compounds containing Si-O-Si bonds are called silicones.<\/p>\n

      \"KSEEB<\/p>\n

      Question 9.
      \nWrite IUPAC name of
      \n\"1st
      \nAnswer:
      \n4 methyl-butan-2-ol.<\/p>\n

      Question 10.
      \nName the organic product obtained when Benzene is treated with excess of chlorine in presence of anhydrous Aluminium chloride.
      \nAnswer:
      \nChlorobenzene.<\/p>\n

      Part – B<\/span><\/p>\n

      II. Answer any FIVE of the following questions carrying TWO marks: ( 5 \u00d7 2 = 10 )<\/span><\/p>\n

      Question 11.
      \nA solution is prepared by adding 2g of a substance A to 18 g of water. Calculate the mass percent of the solute.
      \nAnswer:
      \n\"1st<\/p>\n

      Question 12.
      \nDerive the relation between Density and Molar mass of a gaseous substance from ideal gas equation.
      \nAnswer:
      \nW.K.T PV =- nRT
      \n\"1st
      \nWhere \u03c1 = density, P = Pressure of a gas, M = Molar Mass of gas,
      \nR = gas constant, T = Kelvin Temperature.<\/p>\n

      \"KSEEB<\/p>\n

      Question 13.
      \nWrite the resonance structures of ozone.
      \nAnswer:
      \n\"1st<\/p>\n

      Question 14.
      \nWhat happens when
      \n(i) Quicklime is heated with silica.
      \n(ii) Sodium burns vigorously in oxygen.
      \nAnswer:
      \n(i) Calcium silicate is formed. CaO + SiO2<\/sub> \u2192 CaSiO3<\/sub>
      \n(ii) Sodium bums vigorously in oxygen.
      \n\"1st<\/p>\n

      Question 15.
      \nDiamond is covalent, yet it has high melting point. Why?
      \nAnswer:
      \nDue to strong covalent bonds holding all the carbon atoms in diamond together.<\/p>\n

      Question 16.
      \nHow do you prepare Benzene from Ethyne.
      \nAnswer:
      \nWhen ethyne is passed through a red hot copper tube, it polymerises to form benzene.
      \n\"1st<\/p>\n

      Question 17.
      \nExplain the Friedel crafts alkylation of Benzene with the equation.
      \nAnswer:
      \nWhen Benzene is treated with an alkylhaiide in presence of anhydrous Aluminium Chloride, alkylation takes place to give alkyl benzene.
      \n\"1st<\/p>\n

      Question 18.
      \nWhat are particulate pollutants? Give an example.
      \nAnswer:
      \nParticulate pollutants are solid particles in the air. Example: dust, fumes, mist, smoke.<\/p>\n

      \"KSEEB<\/p>\n

      Part – C<\/span><\/p>\n

      III. Answer any FIVE of the following questions carrying THREE marks: ( 5 \u00d7 3 = 15 )<\/span><\/p>\n

      Question 19.
      \n(a) Define Electro negativity. How does it vary along a group?
      \nAnswer:
      \nThe ability of an atom to attract the shared electron pair (of a covalent bond) in a molecule towards itself is called electro negativity. In a period from left to right the electro negativity increases. Down a group electronegativity value decreases.<\/p>\n

      (b) Which of the following will have most negative electron gain enthalpy?
      \nP, S, Cl, F
      \nAnswer:
      \nF.<\/p>\n

      Question 20.
      \nExplain SP-hybridisation in BeCl2<\/sub> molecule.
      \nAnswer:
      \n\"1st
      \nOne 2S and one 2P orbital of Beryllium undergoes SP hybridisation giving rise to two SP hybrid orbitals of same energy. Which has a linear structure. Two SP hybrid orbitals of Beryllium overlaps with 2P orbital of Chlorine to form two Be-Cl covalent bonds with a bond angle of 180\u00b0.
      \n\"1st<\/p>\n

      Question 21.
      \n(a) Write any two differences between sigma-bond and Pi-bond.
      \n(b) Name the type of Hydrogen bonding in ortho-nitrophenol.
      \nAnswer:
      \n(a)
      \n\u03c3 bond :<\/p>\n

        \n
      1. Overlapping is along the axis<\/li>\n
      2. Overlapping is maximum<\/li>\n
      3. Due to maximum overlap the bond is strong<\/li>\n
      4. s-orbital can participate<\/li>\n<\/ol>\n

        \u03c0 bond :<\/p>\n

          \n
        1. Overlapping is on side wise<\/li>\n
        2. Overlapping is minimum<\/li>\n
        3. Due to minimum overlap, the band is weak<\/li>\n
        4. s-orbital cannot participate<\/li>\n<\/ol>\n

          (b) Intramolecular hydrogen bonding.<\/p>\n

          Question 22.
          \nWrite the Electronic configuration of Oxygen molecule. Predict its magnetic property and calculate its Bond order.
          \nAnswer:
          \nAtomic number of oxygen is 8: 1s2<\/sup> 2s2<\/sup>, 2P4
          \n<\/sup>\"1st
          \n(a) Bond order = \\(\\frac{8-4}{2}\\) = 2
          \n(b) Electronic configuration of oxygen molecule is
          \nKK\u03c32s2<\/sup> \u03c3*2s2<\/sup> \u03c32pz<\/sub>2<\/sup> \u03c02px<\/sub>1 <\/sup>\u03c02p2<\/sup>y <\/sub>\u03c0*2p1<\/sup>x<\/sub> \u03c0*2p1<\/sup>y<\/sub>
          \n(c) Magnetic property: Paramagnetic.<\/p>\n

          Question 23.
          \nBalance the Redox-reaction by using Oxidation number method in acidic medium
          \n\"1st
          \nAnswer:
          \nCr2<\/sub>O2-<\/sup>7<\/sub> + SO3<\/sub>2-<\/sup> \u2192 Cr3+<\/sup>+ SO4<\/sub>-2<\/sup> (Acidic medium)
          \nStep 1.
          \n\"1st<\/p>\n

          Multiply reduction equation by 1 unit and oxidation equation by 3 units
          \nCr2<\/sub>O2-<\/sup>7<\/sub> \u2192 2Cr3+<\/sup>
          \n3SO3<\/sub>2-<\/sup> \u2192 3SO4<\/sub>-2<\/sup>
          \nAdding both equations Cr2<\/sub>O2-<\/sup>7<\/sub> + 3SO3<\/sub>2-<\/sup> \u2192 2Cr3+<\/sup> + 3SO4<\/sub>2-<\/sup>
          \nsince there are 4 oxygen atom more on LHS, 4H2<\/sub>O is added on RHS. The equation is balanced WRT H+<\/sup> ion.
          \nCr2<\/sub>O2-<\/sup>7<\/sub> + 3SO3<\/sub>2-<\/sup> + 8H+<\/sup> \u2192 2Cr3+<\/sup> + 3SO4<\/sub>2-<\/sup> + 4H2<\/sub>O<\/p>\n

          Question 24.
          \n(a) How temporary Hardness of water is removed by Boiling?
          \nAnswer:
          \nHard water can be softened by the following methods depending upon the nature of hardness. Temporary hardness: (i) By boiling: It can be removed by merely boiling the water. Boiling decomposes the bicarbonates to give carbon dioxide and insoluble carbonates, which can be removed by filtration.
          \n\"1st<\/p>\n

          (b) What is the composition of water gas?
          \nAnswer:
          \nCO + H2<\/sub><\/p>\n

          Question 25.
          \n(a) Complete the following reactions.
          \n\"1st
          \nAnswer:
          \n\"1st<\/p>\n

          (b) Lithium shows diagonal relationship with Magnesium. Give reason.
          \nAnswer:
          \nSmall size and high charge density.<\/p>\n

          \"KSEEB<\/p>\n

          Question 26.
          \n(a) Write the chemical formula of Inorganic benzene.
          \nAnswer:
          \nB3<\/sub>N3<\/sub>H6<\/sub>.<\/p>\n

          (b) Write the dimeric structure of Aluminium chloride.
          \nAnswer:
          \n\"1st<\/p>\n

          (c) Define catenation.
          \nAnswer:
          \nCarbon atoms have a remarkable property of joining with one another in a large number to form a long chain and rings. This property is known as catenation or self linkage.<\/p>\n

          Part – D<\/span><\/p>\n

          IV. Answer any FIVE of the following questions carrying FIVE marks: ( 5 \u00d7 5 = 25 )<\/span><\/p>\n

          Question 27.
          \n(a) Calculate the amount of carbon dioxide produced by the combustion of 24g of methane.
          \nAnswer:
          \n\"1st<\/p>\n

          (b) Define Mole. What is the value of Avagadro’s Number.
          \nAnswer:
          \nMass of a substance which contains avogadro number of particles.
          \nAvogadro number = 6.023 x 1023<\/sup><\/p>\n

          (c) Express the number 232.508 in scientific notation.
          \nAnswer:
          \n232.51.<\/p>\n

          Question 28.
          \n(a) What are the observations made in Rutherford a-particle experiment.
          \nAnswer:
          \nThe observations of p ray scattering experiments:<\/p>\n

            \n
          1. About 99% of \u03b1 particles are simply passed through the gold leaf as if they did not come across any obstruction in their path.<\/li>\n
          2. A small number of them got deflected by small angles.<\/li>\n
          3. About 1 out of 20,000 \u03b1 particles got deflected by more than 90\u00b0. A few of them even retracted their path.<\/li>\n<\/ol>\n

            (b) Give any two postulates of Bohr\u2019s theory of Atomic model.
            \nAnswer:
            \nBohr\u2019s model of an atom, the postulates are:<\/p>\n

              \n
            1. Electrons revolve around the nucleus of an atom in a certain definite path called orbit or stationary state of shell.<\/li>\n
            2. The shells are having different energy levels denoted as K, L, M, N…<\/li>\n
            3. As long as the electron remains in an orbit, they neither absorb nor emit energy.<\/li>\n
            4. The electron can move only in that orbit in which angular momentum is quantized,
              \ni.e., the angular momentum of the electron is an integral multiple of \\(\\frac{h}{2 \\pi}\\)<\/li>\n<\/ol>\n

              Question 29.
              \n(a) Name any three quantum numbers and write their significance.
              \nAnswer:
              \n(i) Principal Quantum number : Determines energy and size of the orbital.
              \n(n)
              \n(ii) Azimuthal Quantum number : Determines the shape of the orbitals (sub-shells).
              \n(l)
              \n(iii) Magnetic Quantum number : Determines the orientation of the orbitals.
              \n(m)
              \n(iv) Spin Quantum number : Determines the spin motion of the orbitals.
              \n(s)<\/p>\n

              (b) State heisenberg’s uncertainty principle. Write its mathematical equation.
              \nAnswer:
              \nIt is impossible to determine both the momentum (particle nature) and position (wave nature) of a moving sub atomic particle simultaneously with absolute accuracy.
              \nMathematically \u2206x \u00d7 \u2206p = h \/ 4\u03c0 where Ax = uncertainty in position:
              \n\u2206p = uncertainty in momentum; h = Plank\u2019s constant = 6.626 \u00d7 10-34<\/sup> Js.<\/p>\n

              \"KSEEB<\/p>\n

              Question 30.
              \n(a) Write any three postulates of Kinetic theory of gases.
              \nAnswer:<\/p>\n

                \n
              1. Gases are made up of large number of the minute particles.<\/li>\n
              2. Pressure is exerted by a gas.<\/li>\n
              3. There is no loss of kinetic theory.<\/li>\n
              4. Molecules of gas attract on one another.<\/li>\n<\/ol>\n

                (b) Define critical temperature. Write the value of critical temperature for CO2<\/sub>.
                \nAnswer:
                \nThe maximum temperature at which a gas can be converted into liquid by applying pressure.
                \nCritical temperature of C2<\/sub>\u2192 30.98\u00b0C.<\/p>\n

                Question 31.
                \n(a) Calculate the standard enthalpy of formation of Methane. Given that the standard enthalpy of combustion of Methane, Carbon and Hydrogen are -890.3 kJ,
                \nAnswer:
                \nC(S) + 2H2<\/sub>(g) \u2192 CH4<\/sub>(g) \u2206H ….(1)
                \nC(S) + O2<\/sub> (g) \u2192 CO2<\/sub>(g) \u2206H = -393.5kJ ….. (2)
                \nH2<\/sub>(g) + 1\/2 O2<\/sub> (g) \u2192 H2<\/sub>O() \u2206H = -285.8kJ …… (3)
                \nCH4<\/sub>(g) + 2O2<\/sub> (g) \u2192 CO2<\/sub>(g) + 2H2<\/sub>O(I) \u2206H = -890.3kJ ….. (4)
                \nEqn. (2) \u00d7 , Eqn. (3) \u00d7 2, reverse Eqn. (4), add
                \nH2<\/sub>(g) + O2<\/sub>(g) \u2192 2H2<\/sub>O(l) \u2206H = -571.6kJ
                \nCO2<\/sub>(g) + 2H2<\/sub>O(l) \u2192 CH4<\/sub>(g) + 20,(g) \u2206H = +890.3kJ
                \nC(S) + 2H2<\/sub>(g) \u2192 CH4<\/sub>(g) \u2206H = -74.8kJ<\/p>\n

                (b) What is the change in the value of entropy when ice melts to give water.
                \nAnswer:
                \n+ve (or) positive.<\/p>\n

                Question 32.
                \n(a) State Hess’s law of constant heat summation. Illustrate with examples.
                \nAnswer:
                \nHess\u2019s law : Whether a chemical reaction takes place in a single step or in several steps, the \u2018 total change in enthalpy remains the same.
                \nConsider the formation of CO2<\/sub> from C.<\/p>\n

                I Method (Single step): C(s) + O2<\/sub> (g) \u2192 CO2<\/sub>(g); \u2206H = -xkJ
                \nHeat liberated = xkJ<\/p>\n

                II Method (Two step) : C(s) + \\(\\frac{1}{2}\\) O2<\/sub> (g) \u2192 CO(g);\u2206H = -x,kJ
                \nCO(g) +\\(\\frac{1}{2}\\) O2<\/sub>(g) \u2192 CO2<\/sub>(g) ; \u2206H = -x2<\/sub>kJ .
                \nTotal heat liberated = (x1<\/sub> + x2<\/sub> )kJ
                \nAccording to Hess\u2019s law, x = x1<\/sub> + x2<\/sub><\/p>\n

                (b) Mention any two thermodynamic criteria for spontaneous process.
                \nAnsewr:
                \nChange in Enthalpy should be positive and Change in Entropy should be positive.<\/p>\n

                Question 33.
                \n(a) Define Equilibrium constant. Derive an expression for the equilibrium constant Kc<\/sub> for the reaction.
                \nAnswre:
                \nEquilibrium constant (Kc<\/sub>) is defined as the ratio of product of equilibrium concentrations of products to the product of equilibrium concentrations of reactants each concentration term being raised to its stoichiometric coefficient.
                \nConsider the following reaction at equilibrium.
                \naA + bB \u21cc cC + dD
                \nApplying law of mass action
                \nRf<\/sub> \u221d [A]a<\/sup>[B]b<\/sup>
                \nRf<\/sub> = Kf<\/sub>[A]a<\/sup>[B]b<\/sup>
                \nRb<\/sub> \u221d [C]c<\/sup>[D]d
                \n<\/sup>Rb<\/sub> = Kf<\/sub>[C]c<\/sup>[d]d<\/sup>
                \nAt equilibrium
                \nKf<\/sub>[A]a<\/sup>[B]b<\/sup> = Kf<\/sub>[C]c<\/sup>[d]d
                \n<\/sup>KC<\/sub> = \\(\\frac{\\mathrm{K}_{f}}{\\mathrm{K}_{b}}=\\frac{[\\mathrm{C}]^{\\mathrm{C}}[\\mathrm{D}]^{d}}{[\\mathrm{A}]^{\\mathrm{a}}[\\mathrm{B}]^{\\mathrm{b}}}\\)<\/p>\n

                (b) What is the effect of increase in temperature for the reaction?
                \n2NO2(g)<\/sub> \u21cc N2(g)<\/sub>O4<\/sub>(g); \u2206H = -572.RJ
                \nAnswer:
                \nIncrease in temperature increases the rate of backward reaction because forward reaction is exothermic.<\/p>\n

                (c) Write the relationship between the solubility and solubility product of AB type salt.
                \nAnswer:
                \nKSp<\/sub> = S2<\/sup> (or) S = \u221aKSp<\/sub><\/p>\n

                Question 34.
                \n(a) Calculate the pH of 0.001 M NaOH. Assuming complete dissociation of base.
                \nAnswer:
                \n[OH–<\/sup> ] = 10-3<\/sup> M pOH = -log[10-3<\/sup>] = 3
                \npH + pOH = 14 pH = 14 – 3 = 11<\/p>\n

                (b) Classify the following species into Lewis acid and Lewis base.
                \n(i) HO–<\/sup> (ii) BCl3<\/sub>
                \nAnswer:
                \n(i) HO–<\/sup> \u2192 Lewis base (ii) BCl3<\/sub> \u2192 Lewis acid
                \n(c) Give an example for basic buffer.
                \nAnswer:
                \nNH4<\/sub>Cl + NH4<\/sub>OH<\/p>\n

                \"KSEEB<\/p>\n

                Part – E<\/span><\/p>\n

                V. Answer any TWO of the following questions earning FIVE marks: ( 2 x\u00a05 = 10 )<\/span><\/p>\n

                Question 35.
                \n(a) Explain Functional isomerism with an example.
                \nAnswer:
                \nTwo or more compounds having same molecular formula but different functional groups are called functional isomers. Ex: C3<\/sub>H6<\/sub>O
                \n\"1st<\/p>\n

                (b) For the compound. CHsC-CH = CH CH3<\/sub>
                \n(i) Write the bond line formula for the compound.
                \n(ii) Identify the number of Sigma and Pi-bonds.
                \nAnswer:
                \n\"1st<\/p>\n

                (c) What are free radicals?
                \nAnswer:
                \nA free radical can be defined as an atom or group of atoms having an odd or unpaired electron. Putting a dot (\u2022) against the symbol of atom or group of atoms.
                \n\"1st<\/p>\n

                Question 36.
                \n(a) How do you estimate carbon and hydrogen present in the organic compound by Leibigs method. (Diagram not necessary)
                \nAnswer:
                \nPrinciple: A known mass of an organic compound is strongly heated with dry cupric oxide (CuO), when carbon and hydrogen are quantitatively oxidized to CO2<\/sub> and H2<\/sub>O respectively. The masses of CO2<\/sub> and H2<\/sub>O thus formed are determined. From this, the percentages of carbon and hydrogen can be calculated.<\/p>\n

                Procedure : Pure and dry oxygen is passed through the entire assembly of the apparatus (Figure) till the CO2<\/sub> and moisture is completely removed.
                \n\"1st<\/p>\n

                A boat containing weighed organic substances is introduced inside from one end of the combustion tube by opening it for a while. The tube is now strongly heated till the whole of the organic compound is burnt up. The flow of oxygen is continued to drive CO2<\/sub> and water vapours completely to the U-tubes. The apparatus is cooled and the U-tubes are weighed separately.<\/p>\n

                Observation and calculations:<\/p>\n

                  \n
                1. Mass of organic compound taken = w.g.<\/li>\n
                2. Mass of water produced = x g (Increase in mass of CaCl2 <\/sub>tube).<\/li>\n
                3. Mass of carbon dioxide produced = y g (Increase in mass of KOH tube).<\/li>\n<\/ol>\n

                  To determine % of carbon:
                  \nMolar mass of CO2<\/sub> = 44g mol-1<\/sup>
                  \nNow, 44g of CO2<\/sub> = contains 12 g of C
                  \ny g of CO2<\/sub> will contain of \\(\\frac{12 y}{44}\\) f of C
                  \nThis amount of carbon was present in w. g. of the substance
                  \n\u2234 % C = \\(\\frac{12 y}{44} \\times \\frac{100}{w}\\)<\/p>\n

                  To determine % of Hydrogen
                  \nMolar mass of water = 18 g mol-1<\/sup>
                  \nNow, 18 g of H2<\/sub>O contains 2 g of H2<\/sub>O
                  \n\u2234 x g of H2<\/sub>O will contain \\(\\frac{2 x}{18}\\) g of H2<\/sub>O
                  \nThis amount of hydrogen was present in weight of substance.
                  \n\u2234 H2<\/sub> = \\(\\frac{2 x}{18} \\times \\frac{100}{w}\\)<\/p>\n

                  (b) What are nucleophiles? Give one example.
                  \nAnsert:
                  \nThe molecules or negatively charged ions w hich are capable of donating an electron pair to \u2022 electron deficient centre of the substrate are called nucleophiles.
                  \n\"1st<\/p>\n

                  \"KSEEB<\/p>\n

                  Question 37.
                  \n(a) Explain Free radical mechanism of chlorination of methane.
                  \nAnswer:
                  \nMechanism of chlorination of methane involves three types:<\/p>\n

                  Step 1: Initiation: Chlorine absorbs energy and undergoes homolysis to give chlorine free radicals.
                  \n\"1st<\/p>\n

                  Step 2: Propagation: Chlorine free radical reacts with methane to give methyl free radical.
                  \n\"1st
                  \nThe methyl free radical reacts with chlorine to form methyl chloride and chlorine free radical.
                  \n\"1st<\/p>\n

                  Step 3: Termination: Free radials combine to form stable products.
                  \n\"1st<\/p>\n

                  (b) Complete the following reaction.
                  \n(i) CaC2<\/sub> + 2H2<\/sub>O \u2192 _____ + ______
                  \nAnswer:
                  \n\"1st
                  \n(ii)
                  \n\"1st
                  \nAnswer:
                  \n\"1st<\/p>\n","protected":false},"excerpt":{"rendered":"

                  Students can Download 1st PUC Chemistry Previous Year Question Paper March 2019 (North), Karnataka 1st PUC Chemistry Model Question Papers with Answers helps you to revise the complete Karnataka State Board Syllabus and score more marks in your examinations. Karnataka 1st PUC Chemistry Previous Year Question Paper March 2019 (North) Time: 3.15 Hours Max Marks: …<\/p>\n","protected":false},"author":5,"featured_media":0,"comment_status":"open","ping_status":"open","sticky":false,"template":"","format":"standard","meta":{"footnotes":""},"categories":[81],"tags":[],"jetpack_sharing_enabled":true,"jetpack_featured_media_url":"","_links":{"self":[{"href":"https:\/\/kseebsolutions.guru\/wp-json\/wp\/v2\/posts\/21706"}],"collection":[{"href":"https:\/\/kseebsolutions.guru\/wp-json\/wp\/v2\/posts"}],"about":[{"href":"https:\/\/kseebsolutions.guru\/wp-json\/wp\/v2\/types\/post"}],"author":[{"embeddable":true,"href":"https:\/\/kseebsolutions.guru\/wp-json\/wp\/v2\/users\/5"}],"replies":[{"embeddable":true,"href":"https:\/\/kseebsolutions.guru\/wp-json\/wp\/v2\/comments?post=21706"}],"version-history":[{"count":0,"href":"https:\/\/kseebsolutions.guru\/wp-json\/wp\/v2\/posts\/21706\/revisions"}],"wp:attachment":[{"href":"https:\/\/kseebsolutions.guru\/wp-json\/wp\/v2\/media?parent=21706"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/kseebsolutions.guru\/wp-json\/wp\/v2\/categories?post=21706"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/kseebsolutions.guru\/wp-json\/wp\/v2\/tags?post=21706"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}