3.1.2 - AMOUNT OF SUBSTANCE

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21 Terms

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Mole definition

Unit of measurement of amount of substance

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Avogadro’s constant

Number of particles in a mole

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Formula for number of particles

Num of particles = Moles * Avogadro’s constant

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Formula for moles

Moles = mass (g) / M

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Formula for concentration of solution

Moles = conc. (mol dm⁻³) * volume (dm³)

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Ideal gas equation

pV = nRT

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What does each symbol in ideal gas equation stand for?

p = pressure (Pa)

V = volume (m³)

n = num of moles

R = gas constant

T = temp. (K)

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Empirical formula definition

Smallest whole number ratio of atoms of each element in a compound

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Example empirical formula calculation

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Molecular formula

Gives the actual numbers of atoms of each element in a compound

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Relationship between molecular and empirical formula

Molecular formula is made up of a whole number of empirical units

<p>Molecular formula is made up of a whole <strong>number </strong>of <strong>empirical units</strong></p>
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Ionic equations

  • Can be written for any reaction involving ions that happens in solution

  • Only includes reacting particles (and the products they form)

  • Charges must be balanced on either side

<ul><li><p>Can be written for any reaction involving <strong>ions </strong>that happens in <strong>solution</strong></p></li><li><p>Only includes <strong>reacting particles</strong> (and the <strong>products </strong>they form)</p></li><li><p><strong>Charges </strong>must be <strong>balanced</strong> on either side</p></li></ul><p></p>
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What is a spectator ion?

Ion that’s present in reaction mixture, but not involved in reaction

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What is theoretical yield?

Mass of product that should be formed in reaction - assuming no chemicals are lost in process

Calculated using masses of reactants and balanced equation

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Actual yield is always ____ than theoretical yield

less

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Reasons why actual yield may be less than theoretical

  • Not all reactants react fully

  • Some reactants lost, e.g. lost during transfer between containers

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Formula for percentage yield

Percentage yield = Actual yield / Theoretical yield * 100

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Atom economy definition

A measure of the proportion of reactant atoms that become part of desired product (rather than by-products)

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Formula for atom economy

% atom economy = Mᵣ of desired product / sum of Mᵣ of all reactants * 100

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Example atom economy calculation

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Advantages of processes with high atom economies

  • Better for environment - less waste

  • More sustainable - make more efficient use of raw materials

  • Less expensive - less money spent on separating waste from desired product