Chemistry Chapter: Conservation and Conversions

<p>By dividing actual yield by theoretical yield and multiplying by 100. (C)</p> Signup and view all the answers

<p>When side reactions occur during the process. (A)</p> Signup and view all the answers

<p>50% (B)</p> Signup and view all the answers

<p>Percentage Yield = (actual yield / theoretical yield) × 100 (C)</p> Signup and view all the answers

<p>A substance that is formed during the reaction. (D)</p> Signup and view all the answers

<p>0.03 mol (B)</p> Signup and view all the answers

<p>0.1 mol (D)</p> Signup and view all the answers

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

<p>132 g/mol (D)</p> Signup and view all the answers

<p>3.41 g (B)</p> Signup and view all the answers

<p>Dividing grams of Al by its molar mass (D)</p> Signup and view all the answers

<p>3:1 ratio (B)</p> Signup and view all the answers

<p>Increasing NaCl concentration (D)</p> Signup and view all the answers

<p>Limiting reactants are calculated based on stoichiometric ratios. (C)</p> Signup and view all the answers

<p>The amount of matter remains constant before and after a reaction. (D)</p> Signup and view all the answers

<p>6 moles O2 (C)</p> Signup and view all the answers

<p>The reactant that is fully consumed in a chemical reaction. (A)</p> Signup and view all the answers

<p>To convey the proportions of reactants and products involved. (C)</p> Signup and view all the answers

<p>The ratio of actual yield to theoretical yield multiplied by 100. (C)</p> Signup and view all the answers

<p>The coefficients in the balanced chemical equation. (C)</p> Signup and view all the answers

<p>They remain unreacted after the reaction is complete. (B)</p> Signup and view all the answers

<p>16 moles NH3 (C)</p> Signup and view all the answers

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

<p>The molar mass of the substance (B)</p> Signup and view all the answers

<p>6 moles (D)</p> Signup and view all the answers

<p>31.8 g/mol (A)</p> Signup and view all the answers

<p>Step 3 (A)</p> Signup and view all the answers

<p>42.8 g (B)</p> Signup and view all the answers

<p>Conversion of grams to moles of the first substance (D)</p> Signup and view all the answers

<p>4 moles NH3 to 3 moles O2 (A)</p> Signup and view all the answers

<p>Balancing the chemical equation (C)</p> Signup and view all the answers

<p>Use the molar mass to convert to grams (D)</p> Signup and view all the answers

<p>The average atomic mass of oxygen (A)</p> Signup and view all the answers

<p>42.8 g (C)</p> Signup and view all the answers

<p>Moles of O2 increase (C)</p> Signup and view all the answers

<p>To ensure the conservation of mass (A)</p> Signup and view all the answers

The principle that the total amount of matter remains constant during a chemical reaction.

Using the ratio of moles between substances in a balanced chemical equation to determine the number of moles of one substance given the moles of another.

A chemical equation representing a reaction with equal numbers of atoms of each element on both sides of the equation.

A ratio used to convert from one unit to another, often derived from the balanced chemical equation.

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

The reactant that is not completely consumed in a chemical reaction.

A unit of measurement representing approximately 6.02 x 10^23 particles (atoms, molecules, etc.).

The maximum amount of product that can be formed from a given amount of reactant.

The ratio of the actual yield of a product to the theoretical yield, expressed as a percentage.

Converting the amount of a substance from moles to grams or vice-versa using molar mass.

The mass of one mole of a substance, expressed in grams per mole (g/mol).

The ratio of the coefficients of two substances in a balanced chemical equation, representing their relative amounts in the reaction.

A problem-solving method that uses the units of measurements to guide calculations and conversions.

A substance that takes part in and undergoes change during a reaction.

A substance produced in a chemical reaction.

A symbolic representation of a chemical reaction in the form of chemical formulas and coefficients.

A number placed in front of a chemical formula in a chemical equation to indicate the relative number of moles of that substance.

The mass of an atom of a chemical element.

The mass of a molecule relative to the mass of a carbon-12 atom.

A representation of the elements present in a compound and their relative ratios.

The amount of product you actually get in a real-world lab experiment.

To find the limiting reactant, compare the number of moles of each reactant needed for the reaction to occur completely. The reactant with the fewer moles needed is the limiting reactant.

After determining the limiting reactant, use the stoichiometry of the balanced equation to calculate how much of the excess reactant is used up. Subtract that from the initial amount to find the remaining excess reactant.

Once you know which reactant is limiting, use the stoichiometry of the balanced equation to calculate the maximum amount of product you can make from that limiting reactant.

Compare the calculated moles of each reactant after dividing by their respective coefficients in the balanced chemical equation. The reactant with the smallest calculated value is the limiting reactant.

Subtract the moles of the limiting reactant from the initial moles of the excess reactant.

Use stoichiometry to calculate the mass of product formed based on the moles of the limiting reactant.

The study of the quantitative relationships between reactants and products in chemical reactions. It involves using mole ratios to determine the amount of reactants and products.

Converting the mass of a substance from grams to moles or vice-versa using molar mass.