Phase Changes and Separation Techniques Quiz
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Questions and Answers

What is the acceptable range for the absolute value of the coefficient (a) in scientific notation?

  • 0 < a < 1
  • 0 ≤ a < 10
  • 10 ≤ a < 100
  • 1 ≤ a < 10 (correct)

    • What is the term used for the number that occurs before the 10ⁿ part in scientific notation?

  • Mantissa (correct)
  • Exponent
  • Significant Figure
  • Coefficient

    • Which of the following examples represents the number 24327 in scientific notation?

  • 2.4327 x 10³
  • 2.4327 x 10¹⁴
  • 2.4327 x 10⁵
  • 2.4327 x 10⁴ (correct)

    • In the formula for calculating relative atomic mass, what does the symbol Σ represent?

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

    Which of the following is a valid characteristic of the coefficient (a) in scientific notation?

    <p>It can be a decimal number.</p> Signup and view all the answers

    What process describes the change from solid to liquid?

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

    Which method involves the separation of particles based on centrifugal force?

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

    What is the correct term for the process in which a gas turns into a solid?

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

    Which separation technique is based on the different boiling points of components?

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

    Which of the following best defines a physical property?

    <p>A characteristic that can be observed without altering the substance</p> Signup and view all the answers

    What process is used to separate a mixture by passing it through a medium at different rates?

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

    In which process does a solid directly change into a gas?

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

    Which term refers to the chemical breakdown produced by an electric current?

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

    What is the correct conversion for 1 meter in inches?

    <p>39.37 in</p> Signup and view all the answers

    If you add 3.456 and 2.3, what should the final answer be in terms of significant figures?

    <p>5.8</p> Signup and view all the answers

    Which unit is equivalent to a milli?

    <p>10⁻³ base unit</p> Signup and view all the answers

    What is the maximum number of significant figures that can be in the answer when adding the numbers 4.56 and 3.2?

    <p>3</p> Signup and view all the answers

    How many grams are in 1 pound?

    <p>453.5 g</p> Signup and view all the answers

    What is the equivalent amount of 1 liter in quarts?

    <p>1.057 qt</p> Signup and view all the answers

    When performing multiplication, how do you determine the number of significant figures in your final answer?

    <p>Use the number with the least significant figures</p> Signup and view all the answers

    How many centimeters are there in 1 inch?

    <p>2.54 cm</p> Signup and view all the answers

    What is the first step in determining the empirical formula from a compound's composition?

    <p>Convert the mass of each element to moles</p> Signup and view all the answers

    How is the empirical formula determined after finding the moles of each element?

    <p>By dividing the moles by the smallest mole value</p> Signup and view all the answers

    What is the next step after obtaining the empirical formula?

    <p>Calculate the molecular mass of the empirical formula</p> Signup and view all the answers

    If an empirical formula C₆H₈O₃ has a molecular mass of 128.127 g/mol, how would you find the ratio of the molecular mass of a compound with a molar mass of 256.26 g/mol?

    <p>Divide 256.26 g/mol by 128.127 g/mol</p> Signup and view all the answers

    What is the final empirical formula produced when the ratio is found to be 2 for the compound C₆H₈O₃?

    <p>C₁₂H₁₆O₆</p> Signup and view all the answers

    What is the empirical formula for a compound with 52.14% C, 13.13% H, and 34.73% O?

    <p>C2H6O</p> Signup and view all the answers

    How do you calculate the percent by mass of an element in a compound?

    <p>mass of element / mass of the compound × 100%</p> Signup and view all the answers

    What is the formula to find the molar mass of a compound such as FeCl3?

    <p>1(iron molar mass) + 3(chlorine molar mass)</p> Signup and view all the answers

    What percentage by mass of hydrogen is present in water (H2O)?

    <p>11.2%</p> Signup and view all the answers

    Which statement best describes the molecular formula?

    <p>It shows the actual number of atoms of each element in a compound.</p> Signup and view all the answers

    If a compound contains 34.43% by mass of Iron, what is the mass of Iron in 100 g of the compound?

    <p>34.43 g</p> Signup and view all the answers

    How do you find the mole ratio from the calculated moles of each element?

    <p>Divide by the smallest number of moles.</p> Signup and view all the answers

    Which of the following compounds has a molecular mass of approximately 18.02 g/mol?

    <p>H2O</p> Signup and view all the answers

    To find the subscript in an empirical formula when you have decimal mole ratios, what method would you use?

    <p>Multiply each ratio by a common denominator.</p> Signup and view all the answers

    What is the total molar mass of FeCl3?

    <p>162.2 g/mol</p> Signup and view all the answers

    Calculating the percent composition of an element requires which of the following?

    <p>Mass of the element and mass of the compound</p> Signup and view all the answers

    When given a percent composition, the first step in finding the empirical formula is to assume how many grams of the compound?

    <p>100 g</p> Signup and view all the answers

    If the mole ratio for an empirical formula calculation results in 1.999 H, what should it be rounded to?

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

    The molar mass of which of the following elements is closest to the mass of hydrogen?

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

    Study Notes

    Phase Changes

    • Melting: Transition from solid to liquid.
    • Boiling/Evaporation: Transition from liquid to gas.
    • Condensation: Transition from gas to liquid.
    • Sublimation: Transition from solid to gas.
    • Deposition: Transition from gas to solid.

    Separation Techniques

    • Magnetic/Mechanical Separation: Utilizes tools like forceps, sieves, and magnets to separate solid components of mixtures.
    • Centrifugation: Employs centrifugal force to separate particles from solutions based on size, shape, density, or viscosity.
    • Distillation: Separates components based on their vaporization temperatures.
    • Chromatography: Involves separating mixtures by passing them through a medium, causing different rates of movement.
    • Electrolysis: A chemical method that breaks down compounds by passing an electric current through a solution containing ions.
    • Crystallization: Solid formation through freezing, precipitation, or deposition.

    Properties of Matter

    • Physical Property: Can be measured or observed without altering the substance's composition.
    • Chemical Property: Indicates a substance's ability to change its composition under certain conditions.

    Units and Conversions

    • Common unit conversions:
      • 1 m = 39.37 in = 1.094 yd
      • 1 in = 2.54 cm
      • 1 lb = 453.5 g
      • 1 kg = 2.205 lb
      • 1 L = 1.057 qt
      • 1 atm = 760 mmHg = 101.325 kPa

    Significant Figures in Calculations

    • The result should not exceed the number of significant figures present in the least precise value during addition or subtraction.
    • For multiplication and division, round the result based on the number of significant figures in the initial numbers.

    Relative Atomic Mass Calculation

    • Calculated using the formula: [ \text{Relative Atomic Mass} (Ar) = \frac{\sum(\text{Isotopic Mass} \times \text{Relative Abundance})}{100} ]

    Empirical and Molecular Formulas

    • For empirical formula calculation:

      • Assume 100 g of the compound, convert mass percentages to grams, and then to moles.
      • Divide moles by the smallest mole count for the simplest ratio.

    • To find the molecular formula from the empirical formula:

      • Calculate the empirical formula's molar mass.
      • Divide the given molecular mass by the empirical molar mass.
      • Multiply the empirical formula by the resulting ratio.

    Example Calculations for Composition

    • For H2O:

      • Calculate percent by mass of H: [ % \text{ by mass of H} = \frac{2(1.01)}{18.02} \times 100% = 11.2% ]

    • For FeCl3:

      • Calculate total mass, moles of each element, then determine the percent by mass of iron: [ % \text{ by mass of Fe} = \frac{1(55.85)}{162.2} \times 100% = 34.43% ]

    Mole Ratios

    • Mole ratios should be simplified to the nearest whole number or appropriate fraction based on values obtained in calculations.

    Example for Determining Molecular Formula

    • Given an organic compound's percent composition and molecular mass:
      • Example further illustrates steps from empirical to molecular formula, resulting in C₁₂H₁₆O₆ using the given percentage masses for carbon, hydrogen, and oxygen.

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    General Chemistry 1 Reviewer 2024-2025 PDF

    Description

    Test your knowledge on phase changes, separation techniques, and properties of matter. This quiz covers essential concepts like melting, boiling, and various methods for separating mixtures. It's perfect for students studying chemistry in high school or introductory courses.

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