💏Intro to Chemistry Unit 4 – Stoichiometry of Chemical Reactions

Key Concepts and Definitions

• Stoichiometry involves the quantitative study of reactants and products in a chemical reaction
• Balanced chemical equations represent the relative amounts of reactants and products
• Mole is the SI unit used to measure the amount of a substance, equal to $6.022 \times 10^{23}$ particles (Avogadro's number)
• Molar mass is the mass of one mole of a substance, expressed in grams per mole (g/mol)
  • Calculated by adding the atomic masses of all atoms in a compound
• Limiting reactant is the reactant that is completely consumed first, determining the amount of product formed
• Excess reactant is the reactant that remains after the limiting reactant is consumed
• Theoretical yield is the maximum amount of product that can be obtained based on the balanced chemical equation
• Actual yield is the amount of product actually obtained from a reaction
  • Often less than the theoretical yield due to various factors (incomplete reactions, side reactions, losses during purification)

Balancing Chemical Equations

• Chemical equations must be balanced to satisfy the law of conservation of mass
• The number of atoms of each element must be equal on both sides of the equation
• Coefficients are used to balance the equation, not subscripts
  • Coefficients represent the relative number of moles of each substance
• Steps to balance an equation:
  1. Identify the reactants and products
  2. Write the unbalanced equation
  3. Balance the equation by adjusting coefficients
     • Start with the most complex compound or the element that appears in only one compound on each side
• Balanced equations are essential for stoichiometric calculations

The Mole and Avogadro's Number

• The mole is the SI unit for measuring the amount of a substance
• One mole contains $6.022 \times 10^{23}$ particles (atoms, molecules, or formula units)
  • This number is known as Avogadro's number
• Molar mass is the mass of one mole of a substance, expressed in grams per mole (g/mol)
• Molar mass is used to convert between mass and moles of a substance
  • Moles = Mass (g) ÷ Molar Mass (g/mol)
  • Mass (g) = Moles × Molar Mass (g/mol)
• The mole concept is crucial for understanding and performing stoichiometric calculations

Molar Mass and Molecular Weight

• Molar mass is the mass of one mole of a substance, expressed in grams per mole (g/mol)
• For elements, the molar mass is equal to the atomic mass
  • Example: The molar mass of carbon (C) is 12.01 g/mol
• For compounds, the molar mass is the sum of the atomic masses of all atoms in the compound
  • Example: The molar mass of water (H2O) is 18.02 g/mol (2 × 1.01 g/mol for H + 16.00 g/mol for O)
• Molecular weight is the relative mass of a molecule compared to 1/12 the mass of a carbon-12 atom
  • Numerically equal to the molar mass, but without units
• Molar mass and molecular weight are used to convert between mass, moles, and number of particles

Stoichiometric Calculations

• Stoichiometric calculations involve determining the quantities of reactants and products in a chemical reaction
• Use the balanced chemical equation and molar ratios to set up proportions
• Steps for stoichiometric calculations:
  1. Write and balance the chemical equation
  2. Convert given quantities to moles using molar mass
  3. Set up mole ratios based on the balanced equation
  4. Use the mole ratio to calculate the moles of the desired substance
  5. Convert moles of the desired substance to the requested unit (mass, volume, or particles)
• Dimensional analysis is a useful tool for organizing stoichiometric calculations
  • Arrange conversion factors so that units cancel out, leaving the desired unit

Limiting Reactants and Percent Yield

• Limiting reactant is the reactant that is completely consumed first, determining the amount of product formed
• Excess reactant is the reactant that remains after the limiting reactant is consumed
• Steps to determine the limiting reactant:
  1. Calculate the moles of each reactant
  2. Determine the mole ratio of the reactants from the balanced equation
  3. Divide each reactant's moles by its coefficient in the balanced equation
  4. The reactant with the smallest result is the limiting reactant
• Theoretical yield is the maximum amount of product that can be obtained based on the limiting reactant
• Actual yield is the amount of product actually obtained from a reaction
• Percent yield is the ratio of actual yield to theoretical yield, expressed as a percentage
  • Percent Yield = (Actual Yield ÷ Theoretical Yield) × 100%

Real-World Applications

• Stoichiometry has numerous real-world applications in various fields
• In the pharmaceutical industry, stoichiometry is used to determine the quantities of reactants needed to synthesize drugs
  • Example: Aspirin synthesis requires precise amounts of salicylic acid and acetic anhydride
• In environmental chemistry, stoichiometry helps in understanding and controlling pollutants
  • Example: Calculating the amount of carbon dioxide produced from burning a specific amount of fossil fuel
• In the food industry, stoichiometry is used to optimize production processes and ensure consistent product quality
  • Example: Determining the quantities of ingredients needed to produce a desired amount of food product
• Stoichiometry is also crucial in designing and optimizing industrial chemical processes
  • Example: Calculating the amount of raw materials needed and waste generated in a manufacturing process

Common Pitfalls and Tips

• Double-check that the chemical equation is balanced before performing calculations
• Pay attention to units and convert quantities to moles when necessary
• Be careful with significant figures and round the final answer accordingly
• When determining the limiting reactant, compare the mole ratios, not the actual amounts of reactants
• Remember that the actual yield is often less than the theoretical yield due to various factors
  • Incomplete reactions, side reactions, losses during purification, and experimental errors can reduce the actual yield
• Practice dimensional analysis to organize stoichiometric calculations and ensure the correct units
• Review the periodic table and practice calculating molar masses for elements and compounds
• Work through various stoichiometric problems to gain confidence and identify areas for improvement