Chemistry Chapter 3 Quiz

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Questions and Answers

What is the formula weight of NaOH?

  • 23 g
  • 40 g (correct)
  • 36 g
  • 30 g

Why is the formula weight of NaCl not considered a molecular weight?

  • NaCl is a solid at room temperature.
  • It is too heavy to be a molecular weight.
  • It is not derived from atomic weights.
  • Molecules of NaCl do not exist since it is an ionic compound. (correct)

Which step is NOT part of deriving an empirical formula?

  • Divide by the smallest mole value.
  • Determine the percentage of each element. (correct)
  • Multiply to obtain whole numbers if necessary.
  • Convert grams to moles.

What mass does one mole of H2O have?

<p>18.0 g (B)</p> Signup and view all the answers

Given 43.6% P and 56.4% O in a compound, what is the first step to find the empirical formula?

<p>Base calculations on a 100 g sample. (B)</p> Signup and view all the answers

What does stoichiometry primarily deal with in chemical reactions?

<p>Quantitative relationships between elements and compounds (D)</p> Signup and view all the answers

Which principle postulate distinguishes Dalton's atomic theory from earlier beliefs about matter?

<p>Relative masses of atoms can be measured (B)</p> Signup and view all the answers

What does the law of conservation of mass state?

<p>The mass of reactants equals the mass of products in a chemical reaction (A)</p> Signup and view all the answers

According to Dalton's theory, what causes a pure compound to maintain consistent proportions?

<p>Combination of elements in the same ratios by mass (B)</p> Signup and view all the answers

What is the concept of the law of multiple proportions?

<p>Elements can combine in various ratios to form different compounds (D)</p> Signup and view all the answers

Flashcards

Formula Weight

The sum of the atomic weights of all atoms in a chemical formula.

Molecular Weight

The sum of the atomic weights of all atoms in a molecule.

Empirical Formula

The simplest whole-number ratio of atoms of each element in a compound.

Mole

A unit of measurement in chemistry that equals the Avogadro's number of atoms or molecules.

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Deriving Empirical Formula

Determining the simplest ratio of elements in a compound from percentage composition or mass data.

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Stoichiometry

The branch of chemistry that deals with the quantitative relationships between elements and compounds in chemical reactions.

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Dalton's Atomic Theory

A quantitative theory stating that elements are made of atoms, atoms of the same element are identical in mass, and atoms combine in fixed ratios to form compounds.

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Law of Conservation of Mass

The total mass of reactants is equal to the total mass of the products in a chemical reaction.

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Law of Definite Proportions

A pure compound always contains the same elements combined in the same proportion by mass.

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Isotopes

Atoms of the same element with different atomic masses.

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Related Documents

General Chemistry (1) - Benha University Past Paper PDF

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