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Questions and Answers

What is the normality of the solution when 1.26 grams of oxalic acid is dissolved in 250 ml of solution?

  • 0.02
  • 0.05 (correct)
  • 0.04
  • 0.08

    • What is the formula of the compound formed when 1.26 grams of oxalic acid is dissolved in 250 ml of solution and 80 g of oxygen is released?

  • I2O5
  • I2O (correct)
  • I5O3
  • IO

    • What is the vapour density of a gas?

  • 16
  • 32 (correct)
  • 8
  • 40

    • What is the rest mass of an electron in kg?

    <p>9.11 × 10–31 kg</p> Signup and view all the answers

    What is the mass of carbon in 0.5 mol of potassium ferrocyanide?

    <p>36 g</p> Signup and view all the answers

    What is the atomic mass of an element if one atom of it weighs 1.8 × 10–22 g?

    <p>108.36 g</p> Signup and view all the answers

    What is the molality of the solution when 100 ml of ethylalcohol is made up to a litre with distilled water?

    <p>1.11 m</p> Signup and view all the answers

    If 0.1 mol H2SO4 ionises as H2SO4 + 2H2O →2H3O+ + SO42–, what is the total number of ions produced?

    <p>6.02 × 10^22</p> Signup and view all the answers

    What is the volume of carbon monoxide present at STP when 11.207 litres of CO2 is formed at STP?

    <p>22.414 litres</p> Signup and view all the answers

    What is the nature of the resulting solution when 100 ml of M/10 H2SO4 is mixed with 500 ml of M/10 NaOH?

    <p>Basic, N/5</p> Signup and view all the answers

    If a sample of ammonium phosphate, (NH4)3 PO4, contains 3.18 moles of hydrogen atoms, what is the number of moles of oxygen atoms in the sample?

    <p>1.06</p> Signup and view all the answers

    What is the total number of atoms present in 25.0 mg of camphor, C10H16O?

    <p>2.01 × 10^20</p> Signup and view all the answers

    What is the volume of phosgene formed at STP when 11.2 lit of chlorine reacts with carbon monoxide?

    <p>22.4 lit</p> Signup and view all the answers

    What is the mass of CaCl2 required to produce 14.35 gm of AgCl?

    <p>20.5 g</p> Signup and view all the answers

    Which of the following will not have a mass of 10 g?

    <p>0.1 mol CaCO3</p> Signup and view all the answers

    What is the molar mass of the electron in kg mol-1?

    <p>9.11 × 10–31 kg mol–1</p> Signup and view all the answers

    How many moles of oxygen are present in a vessel that can hold 4 grams of oxygen?

    <p>0.25 moles</p> Signup and view all the answers

    What is the molecular weight of HCl?

    <p>36.46 g/mol</p> Signup and view all the answers

    What is the atomic weight of chlorine in grams?

    <p>35.453 g</p> Signup and view all the answers

    What is the ratio of the volume of ammonia to the total volume of reactants at STP in Haber's process?

    <p>One fourth</p> Signup and view all the answers

    Which law is illustrated by the reaction of carbon with sulphur and oxygen?

    <p>Law of multiple proportions</p> Signup and view all the answers

    What is Avogadro's number?

    <p>6.022 × 10^23</p> Signup and view all the answers

    What is the statement that 'the total mass of reactants is always equal to the total mass of products in a chemical reaction' known as?

    <p>Law of conservation of mass</p> Signup and view all the answers

    How many molecules are present in 16 g of CH4?

    <p>1.205 × 10^23 molecules</p> Signup and view all the answers

    Which of the following laws is illustrated by the reaction of an oxide of nitrogen with nitrogen?

    <p>Law of constant proportions</p> Signup and view all the answers

    What is the number of moles of oxygen atoms in 1 mole of CH4?

    <p>0 mole</p> Signup and view all the answers

    What is the law that states that a chemical compound always contains the same proportion of elements by mass?

    <p>Law of definite proportions</p> Signup and view all the answers

    What is the amount of substance in 1 mole of Na?

    <p>6.022 × 10^23 particles</p> Signup and view all the answers

    Which law is illustrated by the reaction of carbon with sulphur and oxygen, where 6g of carbon combines with 32g of sulphur and 12g of carbon combines with 32g of oxygen?

    <p>Law of multiple proportions</p> Signup and view all the answers

    What is the molecular weight of NH3?

    <p>17 g/mol</p> Signup and view all the answers

    What is the law that states that when two elements form more than one compound, the masses of one element that combine with a fixed mass of the other element are in a simple whole-number ratio?

    <p>Law of multiple proportions</p> Signup and view all the answers

    Which of the following reactions illustrates the law of conservation of mass?

    <p>4.4g of an oxide of nitrogen gives 2.24L of nitrogen and 60g of another oxide of nitrogen gives 22.4L of nitrogen</p> Signup and view all the answers

    Which of the following options is always incorrect?

    <p>Mole fraction is always negative</p> Signup and view all the answers

    If equal masses of SO2 and O2 are placed in a flask at STP, which of the following statements is true?

    <p>The number of molecules of O2 is more than SO2</p> Signup and view all the answers

    In the reaction 2Fe2S3 + 6H2O + 3O2 → 4Fe(OH)3 + 6S, which reagent is in excess?

    <p>O2</p> Signup and view all the answers

    What is the molar ratio of cation to anion in an ionic compound?

    <p>1:2</p> Signup and view all the answers

    What is the formula mass of the compound if the atomic masses of metal and non-metal are 138 and 19, respectively?

    <p>176</p> Signup and view all the answers

    Which of the following statements is true about mole fraction?

    <p>All of the above</p> Signup and view all the answers

    What is the number of moles of Fe2S3 that react with 2 moles of H2O and 3 moles of O2?

    <p>4</p> Signup and view all the answers

    What is the limiting reagent in the reaction 2Fe2S3 + 6H2O + 3O2 → 4Fe(OH)3 + 6S?

    <p>Fe2S3</p> Signup and view all the answers

    Study Notes

    Stoichiometry and Concentration Terms

    • Law of conservation of mass: the total mass of reactants is always equal to the total mass of products in a chemical reaction
    • Law of constant proportions: a chemical compound always contains the same proportion of elements by mass
    • Law of multiple proportions: when two elements form multiple compounds, the masses of one element that combine with a fixed mass of the other element are in a simple whole-number ratio
    • Law of reciprocal proportions: when two elements form multiple compounds, the ratio of the masses of the two elements is always the same

    Gas Laws

    • Vapour density of a gas is proportional to its molecular mass
    • One mole of any gas occupies 22.4 L at STP (Standard Temperature and Pressure)

    Chemical Reactions

    • Haber's process: nitrogen combines with hydrogen to form ammonia (NH3)
    • Combustion reaction: carbon combines with oxygen to form carbon dioxide (CO2)
    • Oxidation reaction: carbon monoxide (CO) is completely oxidized to carbon dioxide (CO2)

    Stoichiometry Problems

    • If 4.4 g of an oxide of nitrogen gives 2.24 L of nitrogen, then 60 g of another oxide of nitrogen gives 22.4 L of nitrogen
    • 6 g of carbon combines with 32 g of sulfur to form CS2, and 12 g of carbon combines with 32 g of oxygen to form CO2
    • 10 g of sulfur combines with 10 g of oxygen to form sulfur dioxide

    Atomic Masses

    • One atom of an element weighs 1.8 × 10^-22 g, its atomic mass is 18
    • The rest mass of an electron is 9.11 × 10^-31 kg, and its molar mass is 5.5 × 10^-7 kg mol^-1

    Concentration Terms

    • Normality of a solution is the number of equivalents of the solute per liter of solution
    • Molality of a solution is the number of moles of solute per kilogram of solvent
    • Molarity of a solution is the number of moles of solute per liter of solution

    Chemical Equations

    • The reaction H2SO4 + 2H2O → 2H3O+ + SO42- involves the ionization of sulfuric acid
    • The reaction C + 2H2 → CH4 involves the formation of methane gas
    • The reaction CaCO3 + HCl → CaCl2 + H2O + CO2 involves the reaction of calcium carbonate with hydrochloric acid

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