Chemistry Quiz: Molarity, Mass, and Laws

True (A)

44 u

<p>22.4</p> Signup and view all the answers

<p>Molecular Mass = Sum of atomic masses in a molecule Formula Mass = Sum of atomic masses in a formula unit Molar Mass = Mass of one mole of a substance in grams Avogadro's Number = Number of particles in one mole</p> Signup and view all the answers

<p>58.5 u (D)</p> Signup and view all the answers

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

<p>313.144 x 10^23 atoms</p> Signup and view all the answers

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

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

<p>0.32 M</p> Signup and view all the answers

<p>82.0245</p> Signup and view all the answers

<p>Mass can neither be created nor destroyed. (C)</p> Signup and view all the answers

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

<p>18 g (A)</p> Signup and view all the answers

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

<p>1:2</p> Signup and view all the answers

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

<p>159.5 g/mol</p> Signup and view all the answers

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

<p>Law of Conservation of Mass = Matter cannot be created or destroyed Law of Definite Proportions = Same elements in same proportion by mass Law of Multiple Proportions = Masses in simple whole number ratios Avogadro's Law = Equal volumes of gases contain equal number of molecules</p> Signup and view all the answers

<p>Avogadro's Law (D)</p> Signup and view all the answers

<p>CH4 = 16 g/mol O2 = 32 g/mol CO2 = 44 g/mol H2O = 18 g/mol</p> Signup and view all the answers

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

<p>39.81 g (B)</p> Signup and view all the answers

<p>2:1</p> Signup and view all the answers

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

<p>1 mole</p> Signup and view all the answers

<p>44.8 L (A)</p> Signup and view all the answers

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

<p>64.5%</p> Signup and view all the answers

<p>46</p> Signup and view all the answers

<p>Glucose = CH2O Ethene = CH2 Ethane = CH3</p> Signup and view all the answers

<p>2 moles of O2 (C)</p> Signup and view all the answers

<p>CH2Cl</p> Signup and view all the answers

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

<p>2 moles (B)</p> Signup and view all the answers

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

<p>0.1 M</p> Signup and view all the answers

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

<p>H2 (B)</p> Signup and view all the answers

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

<p>M1V1 = M2V2</p> Signup and view all the answers

A fundamental principle stating that during a chemical reaction, the total mass of the reactants equals the total mass of the products. This means matter is neither created nor destroyed.

This law states that a specific compound always contains the same elements in the same fixed proportion by mass, regardless of the source or method of preparation.

When two elements form multiple compounds, the masses of one element that combine with a fixed mass of the other element are in a simple whole-number ratio.

This law states that the volumes of gases involved in a chemical reaction at constant temperature and pressure are in a simple whole-number ratio.

Avogadro's Law states that equal volumes of all gases, under the same conditions of temperature and pressure, contain the same number of molecules.

The relative atomic mass of an element is the mass of an atom of that element relative to 1/12th the mass of a carbon-12 atom.

The mass of one mole of a substance is called its molar mass.

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

One atomic mass unit is defined as 1/12th the mass of one carbon-12 atom.

The sum of the atomic masses of all the elements in a molecule.

The sum of atomic masses of the elements present in a formula unit of a compound.

The mass of one mole of a substance in grams.

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

The number of atoms in one mole of a substance.

The number of moles of a substance present in a given mass.

The volume occupied by one mole of any gas at standard temperature and pressure (STP), which is 0°C (273.15 K) and 1 atm.

The percentage by mass of each element present in a compound.

The simplest whole number ratio of atoms present in a compound. It represents the smallest unit of a compound.

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

The study of quantitative relationships between reactants and products in chemical reactions.

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

The reactant that is present in excess after the reaction is complete.

The process of converting a chemical equation into a balanced equation, ensuring the number of atoms of each element is equal on both sides of the equation.

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

The maximum amount of product that can be formed in a reaction, determined by the limiting reagent.

A ratio that expresses the amount of product formed from a given amount of reactant.

The actual amount of product obtained in a reaction, which is usually less than the theoretical yield due to various factors.

A way to express the concentration of a substance in a solution, defined as the number of moles of solute per liter of solution.

Describes the amount of substance per unit mass of solvent. It's expressed as moles of solute per kilogram of solvent.

The number of moles of solute dissolved in 1 kg of solvent.

Molarity changes with temperature because volume changes. Molality is independent of temperature because mass remains constant.

A solution with a higher concentration than a standard working solution, used for preparing dilutions.

The number of moles of solute present in 1 liter of solution.

0.50 mol Na2CO3 refers to the amount of substance (0.50 moles), while 0.50 M Na2CO3 refers to the concentration (0.50 moles per liter).