Stoichiometry & Chemical Reactions Quiz

<p>Mixing solutions with ions that remain in solution. (A)</p> Signup and view all the answers

<p>Endothermic (C)</p> Signup and view all the answers

<p>Na+ (D)</p> Signup and view all the answers

<p>The heat released in a combustion reaction. (D)</p> Signup and view all the answers

<p>They create an insoluble solid from ionic solutions. (B)</p> Signup and view all the answers

<p>The reactant present in the smallest stoichiometric amount (C)</p> Signup and view all the answers

<p>By multiplying the number of atoms by the atomic weight and dividing by the molecular weight of the compound (B)</p> Signup and view all the answers

<p>One reactant will remain unreacted (C)</p> Signup and view all the answers

<p>59.5 g (D)</p> Signup and view all the answers

<p>30.0 amu (C)</p> Signup and view all the answers

<p>0.8 moles (B)</p> Signup and view all the answers

<p>10 g (D)</p> Signup and view all the answers

<p>4.2 moles (A)</p> Signup and view all the answers

<p>Adding instead of dividing molecular weight (A)</p> Signup and view all the answers

<p>18.9 g (B)</p> Signup and view all the answers

<p>Decrease the product yield (A)</p> Signup and view all the answers

The number of moles of a substance is directly proportional to the number of molecules of that substance. 1 mole of any substance contains Avogadro's number (6.022 x 10^23) of molecules.

The ratio of the coefficients of two substances in a balanced chemical equation represents the mole ratio between them. This ratio can be used to calculate the amount of one substance produced or consumed given the amount of another substance.

The amount of product formed in a chemical reaction is limited by the reactant that gets completely consumed first. This reactant is called the limiting reactant.

The molecular weight of a molecule is the sum of the atomic weights of all atoms in the molecule. It is expressed in atomic mass units (amu).

The percent composition of a compound refers to the percentage by mass of each element present in the compound.

The heat change accompanying a chemical reaction is called the heat of reaction. It can be either positive (endothermic, heat absorbed) or negative (exothermic, heat released).

The reaction between ions in an aqueous solution is determined by the solubility rules and the formation of precipitates. If the reaction results in the formation of an insoluble compound (precipitate), then the ions will react.

The theoretical yield is the maximum amount of product that can be formed from a given amount of reactants, assuming 100% efficiency. The actual yield is the amount of product that is actually obtained from a reaction.

The amount of product obtained from a chemical reaction, expressed as a percentage of the theoretical yield.

The theoretical maximum amount of product that can be formed from a given amount of reactants, assuming 100% efficiency.

The ratio of the actual yield to the theoretical yield, multiplied by 100%.

A chemical reaction where the reactants are not in the stoichiometric ratio needed for complete conversion, resulting in some reactants being left over.

The mass of a substance that contains 6.022 x 10^23 particles (atoms, molecules, or ions).

The process where ions in a solution break apart from each other due to the interaction with water molecules. For example, when NaOH dissolves in water, it forms Na+ and OH- ions.

A chemical reaction where two ions combine to form an insoluble solid that falls out of solution. An example is mixing AgNO3 and NaCl to form AgCl precipitate.

A chemical reaction where two ions combine to form a gas that bubbles out of the solution. For example, adding baking soda (NaHCO3) to acid produces carbon dioxide gas.

A reaction between an acid and a base, typically forming water and a salt. For example, HCl (acid) reacting with NaOH (base) produces NaCl (salt) and H2O.

A chemical reaction where electrons are transferred between reactants. For example, the reaction of copper with silver ions (Ag+) results in copper ions (Cu2+) and metallic silver.

The amount of heat released during a combustion reaction. For example, burning fuels like propane releases heat, which is the heat of combustion of that fuel.

A reaction that absorbs heat from the surroundings, causing the reaction mixture to get colder. For example, dissolving some salts in water can be endothermic.