Question 1.4 Calculate the amount of carbon dioxide that could be produced when The unit cube length for LiCl (NaCl) is 5.14 °A. (c) CH3-CH2-OH; Calculate the percentage yield when 180 g of chromium are obtained from a reaction between 100 g of aluminium and 400 g of chromium(III) oxide. Cp [H2O(l)] = 75.3 J mol–1 K–1 Cp [H2O(s)] = 3Question 6. 2Al (s) + Cr2O3 (s) 2Cr (s) + Al2O3 (s) (iv) Diamond is used as an abrasive. (ii) 1 mole of carbon is burnt in 16 g of dioxygen. Question 4.3 Write Lewis symbols for the following atoms and ions: 35.5 Calculate the heat released upon formation of 35.2 g of CO2 from carbon and dioxygen gas. 4.0 Explain. Question 2.8 What is the number of photons of light with a wavelength of 4000 pm that provide 1J of energy? Question 10.27 State as to why Calculate the oxidation number of sulphur in the following molecules H2SO3 and Na2S2O3 Get the answers you need, now! Question 2.6 Find energy of each of the photons which The ionization constant of aniline can be taken from Table7. Question 14. Question 3.11 What do you understand by isoelectronic species? Whether you are looking for essay, coursework, research, or term paper help, or with any other assignments, it is no problem for us. (d) CH3CH2OH (ii) Pentene Question 4.4 Draw the Lewis structures for the following molecules and ions : (v) possible at any temperature 1 (b) 1s and 2px ; Question 2.9 A photon of wavelength 4 × 10–7 m strikes on metal surface, the work function of the metal being 2.13 eV. (i) ( ) ( ) 2 2 PbS s + H O aq → Question 4.39 Define hydrogen bond. Question 9.24 Write chemical reactions to show the amphoteric nature of water. (e) Phosphorus and fluorine (ii) CH4 (g) + 2S2 (g) ƒ CS2 (g) + 2H2S (g) (iii) (n-2) f 7 (n-1)d1ns2 for n=6, in the periodic table. (b) alkali metals are prepared by electrolysis of their fused chlorides ? See the answer. Question 8. How does the result support Kekulé structure for benzene? Question 7.46 The ionization constant of acetic acid is 1.74 × 10–5. (iii) When conc. What is the impact of structure on physical properties of two allotropes? (c) K Question 2.39 In Milikan’s experiment, static electric charge on the oil drops has been obtained by shining X-rays. (c) 3 2 2 2 2 CH CH Br + HO− → CH = CH + H O If decomposition is depicted as, PCl5 (g) ƒ PCl3 (g) + Cl2 (g) ΔrH0 = 124.0 kJ mol–1, a) write an expression for Kc for the reaction. Explain why Question 10.8 Explain why can alkali and alkaline earth metals not be obtained by chemical reduction methods? Question 4.35 Use molecular orbital theory to explain why the Be2 molecule does not exist.4.36 Compare the relative stability of the following species and indicate their magnetic properties; 2 2 2 O ,O+ ,O− (superoxide), 2 2 O − (peroxide) Question 9.15 Saline hydrides are known to react with water violently producing fire. Question 3.38 Considering the elements B, Al, Mg, and K, the correct order of their metallic character is : Question 11.31 Write balanced equations for: 19 For the reaction 2 A(g) + B(g) → 2D(g) ΔU 0 = –10.5 kJ and ΔS0 = –44.1 JK–1. 56 g 32 g 88 g 29 Given the standard electrode potentials, K+/K = –2.93V, Ag+/Ag = 0.80V, Hg2+/Hg = 0.79V Mg2+/Mg = –2.37V. (ii) –52.27 kJ mol–1 Question 1.35 Calcium carbonate reacts with aqueous HCl to give CaCl2 and CO2 according to the reaction, CaCO3 (s) + 2 HCl (aq) → CaCl2 (aq) + CO2(g) + H2O(l) What mass of CaCO3 is required to react completely with 25 mL of 0.75 M HCl? 4x = +10. The compound (A) when heated strongly gives (D), which is used to extract metal. Show transcribed image text. Question 12.29 Will CCl4 give white precipitate of AgCl on heating it with silver nitrate? Discuss. (c) H4P2O7 (b) 2p3 (a) OH– (a) Crystallisation 3 6 × 1 0 − 3 moles of ABD. How will they behave with water ? (iv) 28 g 80 g. (a) Which law of chemical combination is obeyed by the above experimental data? Question 12.5 Which of the following represents the correct IUPAC name for the compounds concerned ? 4.16 Write the significance/applications of dipole moment. (iii) Number of molecules of ethane. Write a balanced redox equation for the reaction. Calculate the bond order of : N2, O2, O2 + and O2. Question 2.7 Calculate the wavelength, frequency and wavenumber of a light wave whose period is 2.0 × 10–10 s. Question 10.7 In what ways lithium shows similarities to magnesium in its chemical behaviour? Question 14. Question 9.7 Discuss the consequences of high enthalpy of H–H bond in terms of chemical reactivity of dihydrogen. (ii) Δp = 0 Question 10.20 The hydroxides and carbonates of sodium and potassium are easily soluble in water while the corresponding salts of magnesium and calcium are sparingly soluble in water. Question 2.16 (i) The energy associated with the first orbit in the hydrogen atom is –2.18 × 10–18 J atom–1. Question 8. (iii) using a catalyst ? Question 5.6 The drain cleaner, Drainex contains small bits of aluminum which react with caustic soda to produce dihydrogen. Question 11.5 Is boric acid a protic acid ? (b) Ag+(aq) and Cu(s) Question 4.20 The skeletal structure of CH3COOH as shown below is correct, but some of the bonds are shown incorrectly. It is oxydised by C r 2 O 7 2 − in acid medium. (b) Nuclear charge (Z ) (a) 3 3 2 CH COOH + HO– → CH COO− + H O (For cupric iodate Ksp = 4 × 10–8 ). 23 38. Question 11.24 How would you explain the lower atomic radius of Ga as compared to Al ? Question 7.69 Equal volumes of 0.002 M solutions of sodium iodate and cupric chlorate are mixed together. Question 11.1 Discuss the pattern of variation in the oxidation states of (i) B to Tl and (ii) C to Pb. Question 2.22 Which of the following are isoelectronic species i.e., those having the same number of electrons? H2SO4 (aq) + 2NH3 (g) (NH4)2SO4 (aq) Question 7.58 The solubility of Sr(OH)2 at 298 K is 19.23 g/L of solution. (a) F > Cl > O > N (ii) O has lower Δi H than N and F? (i) magnesium is burnt in air Amount/smallest amount (b) Fe4[Fe(CN)6]3 Question 9.11 What do you understand by the term “non-stoichiometric hydrides”? Δf H0 = –286 kJ mol–1. (f) NaBH4 Both the ionic and full formulae equations in (3) give the same mole ratio. Question 10.23 Why is LiF almost insoluble in water whereas LiCl soluble not only in water but also in acetone ? Question 7.41 The concentration of hydrogen ion in a sample of soft drink is 3.8 × 10–3 M. what is its pH? Question 9.4 How can the production of dihydrogen, obtained from ‘coal gasification’, be increased ? Exercise 6 In the experiment , 1. Question 4.38 Describe the hybridisation in case of PCl5. Why ? (d) Cr2O7 2– + SO2(g) → Cr3+ (aq) + SO4 2– (aq) (in acidic solution) Question 4.28 What is the total number of sigma and pi bonds in the following molecules ? Question 7.57 If 0.561 g of KOH is dissolved in water to give 200 mL of solution at 298 K. Calculate the concentrations of potassium, hydrogen and hydroxyl ions. The oxidation number for the calcium in CaSO4 is 2+, the oxidation number for oxygen is 2-, and the oxidation number for sulfur is 6+. (a) What is common in them? (i) sodium metal is dropped in water ? 6 8 × 1 0 − 8 moles of K 2 C r 2 O 7 were used for 3. (d) dsp2 (c) Cl2O7 (g) + H2O2(aq) → ClO2 –(aq) + O2(g) + H+ A compound of carbon, hydrogen and oxygen contains 40.0% carbon, 6.6% hydrogen and 53.4% oxygen. (iii) 28 g 32 g Question 7.30 At 473 K, equilibrium constant Kc for decomposition of phosphorus pentachloride, PCl5 is 8.3 ×10-3. The total number of electrons that can be accommodated in all the orbitals having principal quantum number 2 and azimuthal quantum number 1 are (a) 2 (b) 4 (c) 6 (d) 8 (1990) 58. Question 10.31 Which one of the following alkali metals gives hydrated salts ? (iii) Starting with 0.5 mol of ethanol and 1.0 mol of acetic acid and maintaining it at 293 K, 0.214 mol of ethyl acetate is found after sometime. (c) form M2– and M4+ ion (a) 2AgBr (s) + C6H6O2(aq) → 2Ag(s) + 2HBr (aq) + C6H4O2(aq) In short: everything you need to pass A-Level Chemistry: This site uses cookies to improve your experience. (v) 6.0012 Question 7.10 At 450K, Kp= 2.0 × 1010/bar for the given reaction at equilibrium. Question 3.29 Write the general outer electronic configuration of s-, p-, d- and f- block elements. If value of Kc is 8.3 × 10–3, what are the concentrations of PCl3 and Cl2 at equilibrium? Calculate threshold frequency (ν0 ) and work function (W0 ) of the metal. What are its consequences? Why ? If not, how can it be made useful? Question 12.8 Identify the functional groups in the following compounds The equilibrium constant, Kc for the reaction at the given temperature is 3.90. Calculate its empirical formula. 5.5 Explain why is sodium less reactive than potassium. Question 3.25 Would you expect the first ionization enthalpies for two isotopes of the same element to be the same or different? Question 6. Question 9.20 Complete the following chemical reactions. How is classical smog different from photochemical smogs? NEW! Question 1.10 In three moles of ethane (C2H6), calculate the following : Question 4.5 Define octet rule. (ii) The algebraic sum of all the oxidation numbers in a compound is zero. = 2.0 Use Poisson distribution to calculate the approximate number of packets containing no defective and two defective blades, in a consignment of 10,000 packets. Ask your question. Question 7.12 A mixture of 1.57 mol of N2, 1.92 mol of H2 and 8.13 mol of NH3 is introduced into a 20 L reaction vessel at 500 K. At this temperature, the equilibrium constant, Kc for the reaction N2 (g) + 3H2 (g) ƒ 2NH3 (g) is 1.7 × 102. Na = 12.1%, Al = 14.2%, Si = 22.1%, O = 42.1%, H2O = 9.48%. 2 For the process to occur under adiabatic conditions, the correct condition is: (a) exhibit oxidation state of +4 only 0.40/0.10 What is the maximum amount of ammonia that can be recovered from 2.00 x 103 kg of ammonium chloride and 500 kg of quicklime? A 10.0 g sample of a compound contained 3.91 g of carbon, 0.87 g of hydrogen and the remainder is oxygen. (i) ns2np4 for n=3 If not in which direction does the reaction tend to proceed to reach equilibrium? Question 7.55 Calculate the hydrogen ion concentration in the following biological fluids whose pH are given below: Question 10.13 Potassium carbonate cannot be prepared by Solvay process. Question 7.20 One of the reaction that takes place in producing steel from iron ore is the reduction of iron(II) oxide by carbon monoxide to give iron metal and CO2. (a) 1s and 1s Question 5.19 A mixture of dihydrogen and dioxygen at one bar pressure contains 20% by weight of dihydrogen. Question 9.26 What is meant by ‘demineralised’ water and how can it be obtained ? (iii) Find (a) the total number and (b) the total mass of protons in 34 mg of NH3 at STP. Question 14. A thermodynamic state function is a quantity Question 3.14 What is the significance of the terms — ‘isolated gaseous atom’ and ‘ground state’ while defining the ionization enthalpy and electron gain enthalpy? Question 8. (b) Human stomach fluid, 1.2 CaO (s) + 3C (s) CaC2 (s) + CO (g) Question28 Dihydrogen gas is obtained from natural gas by partial oxidation with steam as per following endothermic reaction: CH4 (g) + H2O (g) ƒ CO (g) + 3H2 (g) Question 8. PCl5 (g) ƒ PCl3 (g) + Cl2(g) Question 14. Any element A in a compound ABO has oxidation number -n . (iii) 25365 mg 1 Choose the correct answer. Question 14. Question 3.40 Considering the elements F, Cl, O and N, the correct order of their chemical reactivity in terms of oxidizing property is : Cl Amount of S = 5/32 mol = 0.156 mol We write high quality term papers, sample essays, research papers, dissertations, thesis papers, assignments, book reviews, speeches, book reports, custom web content and business papers. Question 7.43 The ionization constant of HF, HCOOH and HCN at 298K are 6.8 × 10–4, 1.8 × 10–4 and 4.8 × 10–9 respectively. Question 2.11 A 25 watt bulb emits monochromatic yellow light of wavelength of 0.57μm. 5 Statues and monuments in India are affected by acid rain. 22 Calculate the entropy change in surroundings when 1.00 mol of H2O(l) is formed under standard conditions. Question 14. Mass /g (ii) B2H6 + H2O → Question 7.56 The pH of milk, black coffee, tomato juice, lemon juice and egg white are 6.8, 5.0, 4.2, 2.2 and 7.8 respectively. -837.8 kJ b. ⦠(iii) Hexyne Calculate the masses of carbon dioxide and water produced when 0.20 g of this substance is subjected to complete combustion. Question 4.30 Which hybrid orbitals are used by carbon atoms in the following molecules ? Calculate the degree of dissociation of acetic acid in its 0.05 M solution. (iii) 1 mL = ...................... L = ...................... dm3 Mass /g We provide detailed revision materials for A-Level Chemistry students (and teachers). This result means that in the given sample there is 0.10 mol of calcium, 0.20 mol of chlorine and 0.40 mol of water. (a) its acidic nature 11 What are the major causes of water pollution? Amount /mol (a) Human muscle-fluid, 6.83 Fill a cup with brimstone and melt it with a gentle heat. What mass of product is formed. Calculate corresponding hydrogen ion concentration in each. Question 4.13 Write the resonance structures for SO3, NO2 and 3 NO− . 19 Balance the following equations in basic medium by ion-electron method and oxidation number methods and identify the oxidising agent and the reducing agent. and why? (ii) Calculate the radius of Bohr’s fifth orbit for hydrogen atom. Question 1.6 Calculate the concentration of nitric acid in moles per litre in a sample which has a density, 1.41 g mL–1 and the mass per cent of nitric acid in it being 69%. Question 12.15 What is the relationship between the members of following pairs of structures ? Excess of chlorine is harmful. How will this concentration be affected if the solution is 0.1M in HCl also ? Question 7.71 What is the maximum concentration of equimolar solutions of ferrous sulphate and sodium sulphide so that when mixed in equal volumes, there is no precipitation of iron sulphide? b) 0.3 g of Ca(OH)2 dissolved in water to give 500 mL of solution. (b) Na (iii) 100 atoms of A + 100 molecules of B Ask question + 100. Calculate the energy required to remove an electron completely from the n = 2 orbit. Justify your answer. (a) [He] 2s1 Question 1.14 What is the SI unit of mass? (iii) Which of the following orbitals are possible? 1 Define environmental chemistry. © 2021 - CBSEPORTAL.COM - India's First Online Community Website For CBSE Students. (iv) giga 10–15 Isthe reaction at equilibrium? Question 6. Calculate the concentration of the anion, the ionization constant of the acid and its pKa . 40.0 0.20/0.10 2 Explain tropospheric pollution in 100 words. 5 The enthalpy of combustion of methane, graphite and dihydrogen at 298 K are, –890.3 kJ mol–1 –393.5 kJ mol–1, and –285.8 kJ mol–1 respectively. (a) radiation from microwave oven (b) amber light from traffic signal (c) radiation from FM radio (d) cosmic rays from outer space and (e) X-rays. (i) CaH2, BeH2 and TiH2 in order of increasing electrical conductance. Find the percentage composition of nitrogen in the compound. Question 6. (c) CO is heated with ZnO; b) what is the value of Kc for the reverse reaction at the same temperature ? H Question 11.36 Thermodynamically the most stable form of carbon i What volume of dihydrogen at 20 °C and one bar will be released when 0.15g of aluminum reacts? (ii) 10.4107 -2 -3 +6 +4 +3 O This problem has been solved! 6 A reaction, A + B → C + D + q is found to have a positive entropy change. (a) the frequency of emission (b) distance traveled by this radiation in 30 s (c) energy of quantum and (d) number of quanta present if it produces 2 J of energy. (c) Sulphates. (a) PCl5 (g) ƒ PCl3 (g) + Cl2 (g) (d) Hydrated alumina is treated with aqueous NaOH solution. (vii) Aluminium wire is used to make transmission cables. A mole of any substance always contains this number (called the Avogadro number) of particles. (iii) ( ) ( ) 3 8 2 catalyst C H g + 3H O g Δ → Calculate the concentrations of strontium and hydroxyl ions and the pH of the solution. \ = 1.51 (c) Na2O and CO2. (i) The oxidation number of hydrogen is always +1. (b) CH3COCH3 The ground state electron energy is –2.18 × 10–11 ergs. Question 7.33 The value of Kc for the reaction 3O2 (g) ƒ 2O3 (g) is 2.0 ×10–50 at 25°C. The volume of the container is suddenly increased. Question 9.25 Write chemical reactions to justify that hydrogen peroxide can function as an oxidising as well as reducing agent. (e) the metal which can form a stable binary halide of the formula MX2(X=halogen). (a) 3 2 3 2 CH CH Br + HS− → CH CH SH 100. Question 7.60 The pH of 0.1M solution of cyanic acid (HCNO) is 2.34. HNO3 can be transported in aluminium container. 5 Calculate the oxidation number of sulphur, chromium and nitrogen in H2SO5, Cr2O7 2– and NO3 –. (iv) 126,000 What inference do you draw about the behaviour of Ag+ and Cu2+ from these reactions ? (i) p-nitrobromobenzene Question 13.6 An alkene ‘A’ contains three C – C, eight C – H σ bonds and one C – C π bond. (a) 6 CO2(g) + 6H2O(l) → C6 H12 O6(aq) + 6O2(g)(b) O3(g) + H2O2(l) → H2O(l) + 2O2(g) Why it is more appropriate to write these reactions as : (a) 6CO2(g) + 12H2O(l) → C6 H12 O6(aq) + 6H2O(l) + 6O2(g) (b) O3(g) + H2O2 (l) → H2O(l) + O2(g) + O2(g) Also suggest a technique to investigate the path of the above (a) and (b) redox reactions. (ii) 5 × 5.364 Question 7.53 Calculate the degree of ionization of 0.05M acetic acid if its pKa value is 4.74. (a) the least reactive element. Which of these has stronger intermolecular forces and why? (b) F > O > Cl > N Question 5.5 Pressure of 1 g of an ideal gas A at 27 °C is found to be 2 bar. (i) BF3 + LiH → (b) sp – sp3 (c) Hexanedial 8 What are the harmful effects of photochemical smog and how can they be controlled? (d) n = 2, l = 1, ml = 0, ms = – ½ Question 8. Explain. (i) 2NOCl (g) ƒ 2NO (g) + Cl2 (g) Determine the value of x in BaCl2.xH2O. (c) Fe3+ (aq) and Cu(s) Al, Cu, Fe, Mg and Zn. A modification of this type of problem is to determine the ratio of the amount of water to the amount of anhydrous compound. Question 11.8 Write reactions to justify amphoteric nature of aluminium. Question 11.15 If B–Cl bond has a dipole moment, explain why BCl3 molecule has zero dipole moment. Question 1.31 How many significant figures should be present in the answer of the following calculations? Question 13.11 What are the necessary conditions for any system to be aromatic?13.12 Explain why the following systems are not aromatic? Molar mass /g mol-1 Calculating empirical formula from the masses of constituents Calculate the concentration of acetate ion in the solution and its pH. 2NH4Cl (s) CaO (s) CaCl2 (s) + H2O (g) + 2NH3 (g) (ii) Z = 92 , A = 233. = 1.0 Write equations wherever necessary. Describe the shapes of sp, sp2, sp3 hybrid orbitals. 2 CuSO4 + 4 HI -----> 2 CuI + 2 H2SO4 + I2 If 10.4 grams of CuSO4 is used, calculate the number of grams of HI needed and the number of grams of each of the products that are produced. (iii) q = 0 Question 11.19 Explain structures of diborane and boric acid. (b) Carbonates (d) 0.002 M KOH (b) K Determine the formula of a mineral with the following mass composition: (a) n = 0, l = 0, ml = 0, ms = + ½ Question 7.62 A 0.02M solution of pyridinium hydrochloride has pH = 3.44. (e) n = 3, l = 3, ml = –3, ms = + ½ An organic compound was analysed and was found to have the following percentage composition by mass: 48.8% carbon, 13.5% hydrogen and 37.7% nitrogen. This is justified because small differences from whole numbers are probably due to experimental error. Question 9.17 Compare the structures of H2O and H2O2. Question 9.19 Consider the reaction of water with F2 and suggest, in terms of oxidation and reduction, which species are oxidised/reduced. 3. (c) H+ 20 For your agricultural field or garden you have developed a compost producing pit. Question 2.27 Give the number of electrons in the species H H andO 2 2 2 + , + (g) H2S2O7 Question 12.4 Give the IUPAC names of the following compounds : Question 9.23 Discuss the principle and method of softening of hard water by synthetic ionexchange resins. 3. (ii) the carriers of the current in the cell, and What will be its degree of ionization if the solution is also 0.01M in sodium phenolate? 1 Assign oxidation number to the underlined elements in each of the following species: Assign the hybridisation of boron in these species. In the above example however we cannot justify rounding off 1.51 to 1 or 2, but we can obtain a simple ratio by multiplying the relative amounts by two. (v) Aluminium alloys are used to make aircraft body. Question 3.36 The size of isoelectronic species — F–, Ne and Na+ is affected by Question 1.34 A welding fuel gas contains carbon and hydrogen only. 10 Calculate the enthalpy change on freezing of 1.0 mol of water at10.0°C to ice at –10.0°C. (a) sp (d) The block indicates value of azimuthal quantum number (l) for the last subshell that received electrons in building up the electronic configuration. 2. Question 12.25 Why is nitric acid added to sodium extract before adding silver nitrate for testing halogens? Question 5.15 Calculate the total pressure in a mixture of 8 g of dioxygen and 4 g of dihydrogen confined in a vessel of 1 dm3 at 27°C. Question 14.18 A large number of fish are suddenly found floating dead on a lake. Question 3.23 How would you react to the statement that the electronegativity of N on Pauling scale is Question 3.0 in all the nitrogen compounds? S and S2–; Al and Al3+; H and H– (ii) sodium metal is heated in free supply of air ? 24 Refer to the periodic table given in your book and now answer the following questions: (i) Conc. Question 9.13 How does the atomic hydrogen or oxy-hydrogen torch function for cutting and welding purposes ? (a) C2H2 (a) Chlorobenzene, 2,4-dinitrochlorobenzene, p-nitrochlorobenzene 23 Chlorine is used to purify drinking water. (c) Cl > F > O > N = 0.40 5.00 g of iron and 5.00 g of sulphur are heated together to form iron(II) sulphide. What is the longest wavelength of light in cm that can be used to cause this transition? Question 2.29 Using s, p, d notations, describe the orbital with the following quantum numbers. Expert Answer 100% (2 ratings) 2 + 4x – 12 = 0. Question 2.20 Calculate the wavelength of an electron moving with a velocity of 2.05 × 107 m s–1. Question 2.45 Arrange the following type of radiations in increasing order of frequency: Mass of FeS = 0.0893 x 88 g = 7.86 g, Exercise 1 1. (v) fuel-cell ? Question 1.28 Which one of the following will have largest number of atoms? x=+6. Question 8. (c) Tin(IV) oxide Calculate the frequency (ν) and wavenumber ( ν ) of the yellow light. (a) (CH3)3C. (b) 2-Hydroxy-1,2,3-propanetricarboxylic acid Justify your answer. (d) Identify the group having metal, non-metal, liquid as well as gas at the room temperature. (b) Magnesium and nitrogen 48.8 (b) valence principal quantum number (n) ‘A’ on ozonolysis gives two moles of an aldehyde of molar mass 44 u. Formula: The oxidation state of an atom is the charge of this atom after ionic approximation of its heteronuclear bonds. (iv) acetophenone? Question 7.32 Predict which of the following reaction will have appreciable concentration of reactants and products: a) Cl2 (g) ƒ 2Cl (g) Kc = 5 ×10–39 b) Cl2 (g) + 2NO (g) ƒ 2NOCl (g) Kc = 3.7 × 108 c) Cl2 (g) + 2NO2 (g) ƒ 2NO2Cl (g) Kc = 1.8 (a) CH3CH=C(CH3)2 N (iii) used to determine pressure volume work Question 3.3 What is the basic difference in approach between the Mendeleev’s Periodic Law and the Modern Periodic Law? 8. (v) Al + NaOH → (iv) = 0 Kp= 10.1 at 400°C (d) n=4; l=3. Question 13.21 Write structures of all the alkenes which on hydrogenation give 2-methylbutane. An ion has 18 electrons in the outermost shell, it is (a) Cu+ (b) Th 4+ + (c) Cs (d) K+ (1990) 59. (a) 0.003 M HCl Question 8. Question 7.16 What is the equilibrium concentration of each of the substances in the equilibrium when the initial concentration of ICl was 0.78 M ? (i) Lawrence Berkeley Laboratory (iii) the temperature is increased ? Question 7.29 Describe the effect of : a) addition of H2 b) addition of CH3OH c) removal of CO d) removal of CH3OH on the equilibrium of the reaction: Solution Question 11.28 When metal X is treated with sodium hydroxide, a white precipitate (A) is obtained, which is soluble in excess of NaOH to give soluble complex (B). 21 The Mn3+ ion is unstable in solution and undergoes disproportionation to give Mn2+, MnO2, and H+ ion. (i) Pent-2-ene Calculate the equilibrium constant. 9 Consider the reactions: (Assume that mass of a neutron = 1.675 × 10–27 kg). Calculate the ionization constant of the acid and its degree of ionization in the solution. Question 12.26 Explain the reason for the fusion of an organic compound with metallic sodium for testing nitrogen, sulphur and halogens. Question 13.16 Addition of HBr to propene yields 2-bromopropane, while in the presence of benzoyl peroxide, the same reaction yields 1-bromopropane. (b) n = 3, l = 0 Question 7.24 Calculate a) ΔG0 and b) the equilibrium constant for the formation of NO2 from NO and O2 at 298K NO (g) + ½ O2 (g) ƒ NO2 (g) where ΔfG0 (NO2) = 52.0 kJ/mol ΔfG0 (NO) = 87.0 kJ/mol ΔfG0 (O2) = 0 kJ/mol Question 6. (iv) 500.0 Question 13.1 How do you account for the formation of ethane during chlorination of methane ? (ii) sodium carbonate (a) MgCO3 If 8 grams of oxygen contain 3.01 X 10 atoms, calculate the number of atoms present in 2 grams of oxygen. Question 1.19 How many significant figures are present in the following? The sum of the oxidation numbers in a monatomic ion is equal to the overall charge of that ion. Give its statement. Question 10.18 Describe two important uses of each of the following : Question 12.19 Describe the method, which can be used to separate two compounds with different solubilities in a solvent S. (i) –74.8 kJ mol–1 (ii) List the quantum numbers (ml and l ) of electrons for 3d orbital. Question 2.31 How many electrons in an atom may have the following quantum numbers?
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