Chemistry Stoichiometry and Reactions
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Questions and Answers

What is the concentration of the dilute H2SO4 solution in mol/dm³?

  • 0.5 mol/dm³
  • 0.1 mol/dm³
  • 0.0744 mol/dm³ (correct)
  • 0.2 mol/dm³

If 3 moles of NaOH are diluted in 1000 cm³ of solution, what will the molarity be?

  • 0.15 mol/dm³
  • 0.2 mol/dm³ (correct)
  • 0.1 mol/dm³
  • 0.3 mol/dm³

What is the total volume of gases if the total moles of gases is 0.25?

  • 6 dm³ (correct)
  • 24 dm³
  • 500 cm³
  • 2 dm³

Which of the following represents the correct conversion from cm³ to dm³?

<p>1000 cm³ = 1 dm³ (B)</p> Signup and view all the answers

What is the concentration of the concentrated H2SO4 provided?

<p>6.2 mol/dm³ (A)</p> Signup and view all the answers

How many moles of NaOH are present in 1000 cm³ of solution with a concentration of 0.2 mol/dm³?

<p>0.2 moles (D)</p> Signup and view all the answers

What would be the concentration of a solution if 0.0744 moles of solute are dissolved in 1 dm³ of solution?

<p>0.0744 mol/dm³ (A)</p> Signup and view all the answers

Calculating with 3.72 x 10^-3 moles of H2SO4 in a certain volume, how would you determine its concentration?

<p>Dividing moles by volume in dm³ (D)</p> Signup and view all the answers

What is the theoretical yield of a substance in the context provided?

<p>209 g (D)</p> Signup and view all the answers

How many moles of O2 are represented in the content?

<p>0.25 mol (D)</p> Signup and view all the answers

What is the purity percentage of Calcium in limestone as indicated?

<p>88.7% (A)</p> Signup and view all the answers

What amount of actual yield of NH3 is presented?

<p>80 dm (C)</p> Signup and view all the answers

What is the significance of the number 6.0218 mentioned in the content?

<p>It is Avogadro's number, used to define the number of particles in a mole. (B)</p> Signup and view all the answers

What volume of gas at rtp is associated with 0.00417 mol of CaCO3?

<p>22.9 dm³ (B)</p> Signup and view all the answers

Calculate the number of moles of CO2 given as 0.00417 mol, as reflecting the quantity produced.

<p>0.417 mol (C)</p> Signup and view all the answers

What does the term 'actual yield' refer to in the context provided?

<p>The amount of product actually obtained from a reaction. (A)</p> Signup and view all the answers

Which of the following correctly defines the term 'molecular formula'?

<p>It indicates the actual number of each type of atom in a molecule. (D)</p> Signup and view all the answers

What is the calculated total volume of gases at rtp for Mg(NO3)2?

<p>102 g (C)</p> Signup and view all the answers

What does a 20g theoretical yield indicate about a reaction?

<p>It is the predicted amount of product that can be formed under ideal conditions. (A)</p> Signup and view all the answers

If the yield is stated as 100, what is the yield percentage given an actual yield of 80?

<p>80% (D)</p> Signup and view all the answers

What is the relationship between the ratio of moles of gases and the volumes of those gases?

<p>They follow the ideal gas law under specific conditions. (B)</p> Signup and view all the answers

What is the purpose of calculating the ratio between moles of gases?

<p>To find the limiting reactant in a chemical reaction. (C)</p> Signup and view all the answers

What can be inferred if the ratio of actual yield to theoretical yield is low?

<p>There may be significant losses or inefficiencies in the reaction. (D)</p> Signup and view all the answers

If the empirical formula of a substance is CH, what is its molecular formula if it consists of 2 empirical units?

<p>C2H2 (B)</p> Signup and view all the answers

Flashcards

Percentage Yield

The ratio between the actual yield of a reaction and the theoretical yield, expressed as a percentage.

Empirical Formula

The smallest whole number ratio of atoms in a compound.

Molecular Formula

The actual number of atoms of each element in a molecule.

Mole

The amount of substance containing as many elementary entities (atoms, molecules, ions, etc.) as there are atoms in 0.012 kilogram of carbon-12.

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Molar Mass (Mr)

The mass of one mole of a substance.

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Concentration

The number of moles of solute per liter of solution.

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Ratio between Moles of Gases and Volumes of Gases

The ratio between the number of moles of gases and the volumes of gases.

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Ratio between Volumes of Gases and Moles of Gases

The ratio between the volumes of gases and the number of moles of gases.

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Actual Yield

The actual amount of product obtained in a chemical reaction.

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Theoretical Yield

The maximum amount of product that could be produced in a chemical reaction based on the amount of limiting reagent.

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Limiting Reagent

The reactant that is completely consumed in a chemical reaction, limiting the amount of product that can be formed.

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Excess Reagent

A substance that is present in a reaction mixture in excess of the amount required to react completely with the limiting reagent.

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Mass of Impure Substance

The mass of a substance that is obtained from a chemical reaction, considering the purity of the starting material.

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Purity

The ratio of the mass of a pure substance to the total mass of the substance, expressed as a percentage.

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Volume at STP

The volume of a gas at standard temperature and pressure (STP).

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Dilution

The process of reducing the concentration of a solution by adding more solvent, usually water.

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Molarity (M)

The number of moles of solute dissolved in one liter (dm³) of solution.

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Titration

The process where a chemical reaction is used to determine the concentration of a solution.

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Redox Reaction

A chemical reaction that involves the transfer of electrons or hydrogen ions between reactants.

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Hydrolysis

A chemical reaction in which a substance reacts with water to form an acid or a base.

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Molar Volume

The volume occupied by one mole of a gas at standard temperature and pressure (STP).

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Study Notes

Stoichiometry Calculations

  • Percentage Yield: (Actual yield / Theoretical yield) x 100
  • Molecular Formula: (Empirical formula)n , where n = Mr / Er
  • Moles of a Gas at RTP: Volume (dm³) / 24
  • Moles of a substance from mass and molar mass: Mass (grams) / Molar mass (g/mol)
  • Ratio between gas moles and volumes is equal: Moles of gas A / Moles of gas B = Volume of gas A / Volume of gas B
  • Ideal Gas Law: (CV) before = (CV) after
  • Actual Yield: The amount of product obtained in a reaction.
  • Theoretical Yield: The maximum amount of product that can be produced in a reaction according to the balanced chemical equation.

Chemical Reactions and Equations

  • Balanced Equation: 2Mg + Oâ‚‚ → 2MgO
  • Moles of Mg reacted = 0.5 mol
  • Moles of MgO formed = 0.5 mol
  • Calculating % Yield: (Actual Yield/Theoretical Yield) * 100%
  • Calculating volume of gases at RTP: (Moles of gas)*24 dm³

Titration Calculations

  • Calculating moles of NaOH: Conc (mol/dm³) x Volume (dm³)
  • Calculating moles of Hâ‚‚SOâ‚„: Conc (mol/dm³) x Volume (dm³)
  • Moles from dilution: Concentrations are related by equations such as CxV = CxV, where C is the concentration and V is the volume with the subscripts referring before and after the dilution
  • Calculating concentration of Hâ‚‚SOâ‚„: Moles / Volume

Other Calculations

  • Calculating moles of CaCO₃ (Using balanced equation & ideal gas Law)
  • Percentage purity: (mass of pure substance/ mass of impure substance)× 100%
  • Empirical & Molecular Formulas: Used for calculating formulae from experimental data
  • Calculations from Reactions involving gases: Stoichiometry is used to determine how much of substances reacts or is produced in chemical equations.

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Description

Test your understanding of stoichiometry, chemical reactions, and titration calculations. This quiz covers key concepts like percentage yield, molecular formulas, and the ideal gas law, providing a comprehensive overview of essential chemistry principles. Perfect for students looking to reinforce their knowledge in these areas.

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