7.7 Mole Relationships in Chemical Equations

7.7 Mole Relationships in Chemical Equations

  • When the reactant that is reduced reacts with hydrogen, it forms a saturated hydrocarbon.

  • The Succinic acid Fumaric acid oxidation and reduction reactions of the iron ion in the cell's cyto are accompanied by a coenzyme, flavin adenine chromes.
  • A strong germicide is used to kill germs in swimming pools.
  • A mole-mole factor can be used to calculate the number of moles of another substance in a reaction.
  • The total amount of matter in the reactants is the same as the total amount of matter in the products.
    • The total mass of the reactants must be the same as the total mass of the products.
    • As original substances are changed to new substances, no material is lost or gained.
  • When silver reacts with sulfur to form silver sulfide, tarnish forms.
  • The mass of the reactants is the same as the mass of the product.
  • The number of silver atoms that react is more than the number of sulfur atoms.
    • 100 sulfur atoms are required when 200 silver atoms react.
    • Many more atoms of both silver and sulfur would react in the chemical reaction.
    • The coefficients in the equation can be interpreted in terms of moles if we are dealing with silver and sulfur.
    • 2 moles of silver react with 1 mole of sulfur to form 1 mole of Ag2S.
    • The moles of Ag, S, and Ag2S can be stated in grams of each because the molar mass of each can be determined.
    • There are 215.8 g of Ag and 32.1 g of S in this picture.
    • The mass of reactants is equal to the mass of product.
  • The product is iron(III) sulfide when iron reacts with sulfur.
  • The balanced chemical equation shows that 2 moles of iron react with 3 moles of sulfur to form 1 mole of iron(III) sulfide.
  • You need to know the correct amount of reactants to use and how much of the product will form if you want to prepare medicines in a pharmaceutical laboratory.
  • There are given and needed quantities.
  • To convert the given to the needed quantity, you have to write a plan.
  • Write mole-mole factors using coefficients.
  • Give the needed quantity by setting up the problem.
  • The number of moles of iron needed to react with sulfur is calculated using the equation.
  • The number of moles of another substance in the water is calculated using the chemical reaction of hydrogen with oxygen.