Chemical Equations

3Fe (s) + Al2(SO4)3 (aq) → 3Fe(SO4) (aq) + 2Al (s)

The balanced chemical equation for the reaction between hypochlorite ion (OCl-) and thiosulfate ion (S2O3^2-) is:

2OCl- + 2S2O3^2- -> 2Cl- + S4O6^2- + 2OH-

The complete chemical equation for photosynthesis is: 6CO2 + 6H2O + light energy → C6H12O6 + 6O2. This equation represents the process by which plants, algae, and some bacteria convert carbon dioxide and water into glucose and oxygen using sunlight as an energy source.

An unbalanced equation (skeleton equation) only indicates the nature of the reactants and products but tells nothing of the stoichiometric ratios, i.e. it tells nothing of how much of each species is present, not which reactant might be in excess or limiting, etc.

To balance a chemical equation, start by counting the number of each type of atom on both sides. Adjust coefficients to make the number of atoms of each element equal on both sides. Begin by balancing elements that appear in only one reactant and one product, then proceed to balance the more complex molecules. Remember to preserve the law of conservation of mass while balancing the equation.

A chemical equation may be written in a balanced form, showing the same number of atoms of each element on both sides, or in an unbalanced form, representing the reactants and products without considering conservation of mass.

The balanced chemical equation for the reaction between barium nitrate (Ba(NO3)2) and potassium hydroxide (KOH) is: Ba(NO3)2 + 2KOH -> Ba(OH)2 + 2KNO3

The balanced chemical equation for burning C18H38 in air is:

2C18H38 + 55O2 → 36CO2 + 38H2O

An unbalanced chemical equation does not accurately reflect the ratio of reactants and products in a chemical reaction, which can affect the stoichiometry of the reaction. Balancing the equation is necessary to ensure that the law of conservation of mass is obeyed and to correctly represent the chemical species involved in the reaction.

Coefficients in a balanced chemical equation provide the relative ratio of reactants and products involved in a chemical reaction. They indicate the number of molecules or moles of each substance that participate in the reaction. Coefficients help to ensure that the law of conservation of mass is satisfied by showing that the same number and types of atoms are present on both sides of the equation.

NiSO4 + Na2(edta) -----> Ni(edta) + Na2SO4

If a chemical equation is not balanced, it violates the Law of Conservation of Mass. This law states that matter cannot be created or destroyed in a chemical reaction, so the number of atoms of each element must be the same on both sides of a balanced chemical equation.

The balanced chemical equation would be: NF3 + F2 -> N + 3F2 The coefficient for fluorine would be 2 and the symbol is F2.

3 Ca(OH)2 + 2 H3PO4 --> Ca3(PO4)2 +6 H2O

Note:

Ca(OH)2 is not very soluble in water but enough to react with the acid, but may be some excess will be needed

Balancing chemical equations is a result of the law of conservation of mass, which states that matter cannot be created or destroyed in a chemical reaction. Balancing the number of atoms on both sides of the equation ensures that the total mass is conserved before and after the reaction.

The formula for barium sulfide is BaS. The gram atomic mass of barium is 137.33 and the gram atomic mass of sulfur is 32.06. Therefore, the mass percent of barium in barium sulfide is 100[137.33/(137.33 + 32.06)] or 81.073 %. (Five significant digits are justified even though the value for sulfur has only four significant digits, because the only use made of the value for sulfur in the calculation is to add it to a number with more significant digits.)

The balanced chemical equation for the reaction between sodium chloride (NaCl) and potassium iodide (KI) is: 2NaCl + KI → NaI + KCl. This equation ensures that there is the same number of each type of atom on both sides of the reaction.

In order to determine the mass of a compound from a chemical equation, you need to look at the chemical formula for the compound you need to find the mass of. Using the periodic table, add up the atomic mass of each atom in the compound. For example, the molar mass of ethane, C2H6, is 12.01+12.01+1.008+1.008+1.008+1.008+1.008+1.008 = 30.068 grams/mole

In order to find the mass of a product in a chemical equation, you need to convert any information you are given into moles. You can use this information to determine how many moles of product are produced using the ratio given by the chemical equation. Then the number of moles of product is converted to mass using the molecular weight of the compound as determined above.

example)

2Na(s) + 2H2O(l) --> 2NaOH(aq) + H2(g)

Find the mass of hydrogen gas produced if 23 grams of sodium react with excess water.

Atomic mass of sodium: 22.99 grams/mol

(23grams)/(22.99grams/mol) = 1 mole sodium

The ratio of sodium to hydrogen gas is 2:1 so:

(1 mol Na) * (1 mol H2)/(2 mol Na) = .5 mol H2

The atomic mass of hydrogen is 1.008, so the molecular weight of H2 is 1.008 +1.008, or 2.016 grams/mol.

(.5 mol H2) * (2.016 grams/mol) = 1.008 grams of hydrogen gas produced.

The balanced chemical equation for the reaction of C2H6O (ethanol) with O2 (oxygen) to form CO2 (carbon dioxide) and H2O (water) is: C2H6O + 3O2 → 2CO2 + 3H2O.

Putting a chemical equation into words helps to describe the reactants, products, and the chemical reaction that is occurring. It allows for easier communication of the reaction process and helps in understanding the stoichiometry involved. Additionally, writing chemical equations in words helps to identify the type of reaction taking place.

The chemical equation for the oxidation of sec-butyl alcohol can be written as:

Sec-butyl alcohol + [O] -> Sec-butyl aldehyde + H2O

A chemical equation contains the symbols and formulas of the reactants and products involved in a chemical reaction, along with the coefficients that represent the relative amounts of each substance. It also shows the state of matter (solid, liquid, gas, aqueous) of each substance and depicts the conservation of mass and atoms in the reaction.