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4 types of chemical equations
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From Wikipedia
A chemical equation is symbolic representation of a chemical reaction where the reactant entities are given on the left hand side and the product entities on the right hand side. The coefficients next to the symbols and formulae of entities are the absolute values of the stoichiometric numbers. The first chemical equation was diagrammed by Jean Beguin in 1615.
Form
A chemical equation consists of the chemical formulas of the reactants (the starting substances) and the chemical formula of the products (substances formed in the chemical reaction). The two are separated by an arrow symbol (\rightarrow, usually read as "yields") and each individual substance's chemical formula is separated from others by a plus sign.
As an example, the formula for the burning of methane can be denoted:
 CH4 + 2 O2 \rightarrow CO2 + 2 H2O
This equation would be read as "CH four plus O two produces CO two and H two O." But for equations involving complex chemicals, rather than reading the letter and its subscript, the chemical formulas are read using IUPAC nomenclature. Using IUPAC nomenclature, this equation would be read as "methane plus oxygen yields carbon dioxide and water."
This equation indicates that oxygen and CH_{4} react to form H_{2}O and CO_{2}. It also indicates that two oxygen molecules are required for every methane molecule and the reaction will form two water molecules and one carbon dioxide molecule for every methane and two oxygen molecules that react. The stoichiometric coefficients (the numbers in front of the chemical formulas) result from the law of conservation of mass and the law of conservation of charge (see "Balancing Chemical Equation" section below for more information).
Common symbols
Symbols are used to differentiate between different types of reactions. To denote the type of reaction:
 "=" symbol is used to denote a stoichiometric relation.
 "\rightarrow" symbol is used to denote a net forward reaction.
 "\rightleftarrows" symbol is used to denote a reaction in both directions.
 "\rightleftharpoons" symbol is used to denote an equilibrium.
Physical state of chemicals is also very commonly stated in parentheses after the chemical symbol, especially for ionic reactions. When stating physical state, (s) denotes a solid, (l) denotes a liquid, (g) denotes a gas and (aq) denotes an aqueous solution.
If the reaction requires energy, it is indicated above the arrow. A capital Greek letter delta (\Delta) is put on the reaction arrow to show that energy in the form of heat is added to the reaction. h\nu is used if the energy is added in the form of light.
Balancing chemical equations
The law of conservation of mass dictates the quantity of each element does not change in a chemical reaction. Thus, each side of the chemical equation must represent the same quantity of any particular element. Similarly, the charge is conserved in a chemical reaction. Therefore, the same charge must be present on both sides of the balanced equation.
One balances a chemical equation by changing the scalar number for each chemical formula. Simple chemical equations can be balanced by inspection, that is, by trial and error. Another technique involves solving a system of linear equations.
Ordinarily, balanced equations are written with smallest wholenumber coefficients. If there is no coefficient before a chemical formula, the coefficient 1 is understood.
The method of inspection can be outlined as putting a coefficient of 1 in front of the most complex chemical formula and putting the other coefficients before everything else such that both sides of the arrows have the same number of each atom. If any fractional coefficient exist, multiply every coefficient with the smallest number required to make them whole, typically the denominator of the fractional coefficient for a reaction with a single fractional coefficient.
As an example, the burning of methane would be balanced by putting a coefficient of 1 before the CH_{4}:
 1 CH4 + O2 \rightarrow CO2 + H2O
Since there is one carbon on each side of the arrow, the first atom (carbon) is balanced.
Looking at the next atom (hydrogen), the right hand side has two atoms, while the left hand side has four. To balance the hydrogens, 2 goes in front of the H_{2}O, which yields:
 1 CH4 + O2 \rightarrow CO2 + 2 H2O
Inspection of the last atom to be balanced (oxygen) shows that the right hand side has four atoms, while the left hand side has two. It can be balanced by putting a 2 before O_{2}, giving the balanced equation:
 CH4 + 2 O2 \rightarrow CO2 + 2 H2O
This equation does not have any coefficients in front of CH_{4} and CO_{2}, since a coefficient of 1 is dropped.
Ionic equations
An ionic equation is a chemical equation in which electrolytes are written as dissociated ions. Ionic equations are used for single and double displacement reactions that occur in aqueoussolutions. For example in the following precipitation reaction:
 CaCl_{2}(aq) + 2AgNO_{3}(aq) \rightarrow Ca(NO_{3})_{2}(aq) + 2AgCl(s)
the full ionic equation would be:
 Ca^{2+} + 2Cl^{−} + 2Ag^{+} + 2NO_{3}^{−} \rightarrow Ca^{2+} + 2NO_{3}^{−} + 2AgCl(s)
and the net ionic equation would be:
 2Cl^{−}(aq) + 2Ag^{+}(aq) \rightarrow 2AgCl(s)
or, in reduced balanced form,
 Ag^{+} + Cl^{−} \rightarrow AgCl(s)
In this aqueous reaction the Ca^{2+} an
From Yahoo Answers
Answers:That is synthesis. When two reactant from a solution. Then there is combustion, decomposition, single replacement and double replacement. Combustion  When organic compounds like propane are burned, they react with the oxygen in the air to form carbon dioxide and water. The reason why these combustion reactions will stop when all available oxygen is used up is because oxygen is one of the reactants. Decomposition: A decomposition reaction is the opposite of a synthesis reaction  a complex molecule breaks down to make simpler ones. These reactions come in the general form: AB > A + B And single and double replacement are just what they sound like.
Answers:i hope you are not expecting anyone to do this assignment FOR you.
Answers:_____PV=nRT Qs and V = n (RT/P) and for CONSTANT P&T, V= kn 1) 3O2 > 2O3; VO2 cm3 = VO3 cm3 * (3moles O2/ 2 moles O3) = ?? 2) 6 O2 > 6 CO2; V CO2 dm3 = VO2 dm3 * (6moles CO2 / 6moles O2) = ?? 3) 3 H2 > 2 NH3; V NH3 liters = VH2 liters * (2 moles NH3 / 3 moles H2) = ?? 4) 1 O2 reacts with 2H2; VO2 cm3 = VH2 cm3 * (1 mole O2 / 2 mole H2) = ?? Plug and SOLVE Basic mathematics is a prerequisite to chemistry I just try to help you with the methodology of solving the problem.
Answers:1) Double replacement, general form is AB + CD > AD + CB 2) Double replacement 3) Double replacement 4) Combustion, because H2O and CO2 are products
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