english for Predict Rendement of Product a l Reaction
Chemistry
students typically experience difficulty in predicting the products of chemical
reactions. With practice, however, the process becomes progressively easier.
The first
step---identifying the type of reaction involved---is usually the most
difficult. The primary reaction types students encounter are displacement,
acid-base and combustion. They are easily identified if the tell-tale signs are
known. Displacement reactions involve two ionic compounds with cations and
anions, such as sodium sulfate, in which sodium (Na?) is the cation and sulfate
(SO?²?) is the anion. Ionic compounds always consist of a metal and a nonmetal
or polyatomic (multiple-atom) anion. Decomposition reactions involve a single
compound breaking into two or more compounds. Acid-base reactions must involve
an acid (identified by its chemical formula that begins with “H,” such as HCl).
Combustion reactions involve hydrogen or a hydrocarbon (such as CH?) reacting
with oxygen (O?).
Displacement Reactions
Identify the
cation and anion of the compounds involved in the reaction, as well as their
charges. If necessary, refer to tables of cations and anions, such as the one
available at Penn State University’s website (See Resources). Sodium chloride
(NaCl), for example, consists of a sodium ion (Na?) and a chloride ion (Cl?).
Exchange the
anions of the two reactants to determine the products of the reaction. Displacement
reactions take this general form:
AB + CD ? AD
+ CB
Thus, for a
reaction between sodium chloride (NaCl) and silver nitrate (AgNO?):
NaCl + AgNO?
? NaNO? + AgCl
Determine
whether the products are soluble. This may require referring to a list of
“solubility rules,” such as that at Southern Methodist University (see
Resources). In the example from Step 2, NaNO? is soluble and thus remains in
solution, but AgCl is insoluble and will form a precipitate.
Verify that
the reaction is balanced by adding coefficients in front of the reactants and
products as necessary to ensure that each type of atom is present on each side
of the reaction arrow in equal numbers. In the example from Step 2, the left
side of the equation contains 1 Na, 1 Cl, 1 Ag, 1 N, and 3 O; the right side
contains 1 Na, 1 Cl, 1 Ag, 1 N, and 3 O. Thus, the reaction is balanced.
Acid-Base Reactions
Identify the
acidic compound (containing H? in its formula) and the basic compound (usually
a hydroxide, OH?).
Determine
the products according to the general reaction:
acid + base
? salt + water
For example,
the reaction of hydrochloric acid (HCl) with sodium hydroxide (NaOH) produces
sodium chloride and water:
HCl + NaOH ?
NaCl + H?O
Determine if
the salt is soluble or insoluble by referring to the solubility rules.
Balance the
reaction. In this case, the reaction from Step 2 is already balanced.
Combustion Reactions
Determine
the fuel (the source of carbon and/or hydrogen) and the oxidant (the source of
oxygen) (see Resources). If the combustion is carried out in air, the oxidant
is assumed to be molecular oxygen (O?). Other oxidants, such as nitrous oxide
(N?O), are possible, but this would require special reaction conditions.
Predict the
products by assuming this general reaction:
Fuel +
oxidant ? CO? + H?O
For example,
propane (C?H?) combines with O? during combustion as:
C?H? + O? ?
CO? + H?O
Balance the
reaction. For the example in Step 2:
C?H? + 5 O?
? 3 CO? + 4 H?O
Predicting Reaction Products - Solutions
Balance the equations and predict the products for the
following reactions:
1) 3 Na + 1 FeBr3 3
NaBr + 1 Fe
2) 2 NaOH + 1 H2SO4
1 Na2SO4 + 2 H2O
3) 1 C2H4O2 + 2 O2
2 CO2 + 2 H2O
4) 1 NH3 + 1 H2O 1
NH4OH
•
STEPS FOR PREDICTING PRODUCTS
Classify the reaction based on the reactants
Classify the reaction based on the reactants
•
Predict the
products based on the type of reaction
•
Write the formula for each product (Take into
consideration type of bonds, polyatomic ions, & diatomic elements)
Balance the chemical equation and use the solubility table to add state
symbols
Diatomics!
• Remember the elements that exist in
diatomic form.
• H, N, O,
F, Cl, Br and I
• All exist
with two of the atoms bonded together:
• H2
N2 O2 F2
Cl2 , Br2 , I2
Polyatomic
Ions!
• MEMORIZE YOUR POLYATOMICS
– Ammonium NH4+1
– Hydroxide
OH-1
– Nitrite NO2-1
– Nitrate NO3-1
– Hydrogen
sulfate HSO4-1
– Hydrogen
carbonate (bicarbonate) HCO3 -1
– Carbonate
CO3-2
– Sulfate SO4-2
– Phosphate
PO4 -3
How
to Predict Products in Chemical Reactions
Chemistry
students typically experience difficulty in predicting the products of chemical
reactions. With practice, however, the process becomes progressively easier.
The first
step---identifying the type of reaction involved---is usually the most
difficult. The primary reaction types students encounter are displacement,
acid-base and combustion. They are easily identified if the tell-tale signs are
known. Displacement reactions involve two ionic compounds with cations and
anions, such as sodium sulfate, in which sodium (Na?) is the cation and sulfate
(SO?²?) is the anion. Ionic compounds always consist of a metal and a nonmetal
or polyatomic (multiple-atom) anion. Decomposition reactions involve a single
compound breaking into two or more compounds. Acid-base reactions must involve
an acid (identified by its chemical formula that begins with “H,” such as HCl).
Combustion reactions involve hydrogen or a hydrocarbon (such as CH?) reacting
with oxygen (O?).
Displacement Reactions
Identify the
cation and anion of the compounds involved in the reaction, as well as their
charges. If necessary, refer to tables of cations and anions, such as the one
available at Penn State University’s website (See Resources). Sodium chloride
(NaCl), for example, consists of a sodium ion (Na?) and a chloride ion (Cl?).
Exchange the
anions of the two reactants to determine the products of the reaction. Displacement
reactions take this general form:
AB + CD ? AD
+ CB
Thus, for a
reaction between sodium chloride (NaCl) and silver nitrate (AgNO?):
NaCl + AgNO?
? NaNO? + AgCl
Determine
whether the products are soluble. This may require referring to a list of
“solubility rules,” such as that at Southern Methodist University (see
Resources). In the example from Step 2, NaNO? is soluble and thus remains in
solution, but AgCl is insoluble and will form a precipitate.
Verify that
the reaction is balanced by adding coefficients in front of the reactants and
products as necessary to ensure that each type of atom is present on each side
of the reaction arrow in equal numbers. In the example from Step 2, the left
side of the equation contains 1 Na, 1 Cl, 1 Ag, 1 N, and 3 O; the right side
contains 1 Na, 1 Cl, 1 Ag, 1 N, and 3 O. Thus, the reaction is balanced.
Acid-Base Reactions
Identify the
acidic compound (containing H? in its formula) and the basic compound (usually
a hydroxide, OH?).
Determine
the products according to the general reaction:
acid + base
? salt + water
For example,
the reaction of hydrochloric acid (HCl) with sodium hydroxide (NaOH) produces
sodium chloride and water:
HCl + NaOH ?
NaCl + H?O
Determine if
the salt is soluble or insoluble by referring to the solubility rules.
Balance the
reaction. In this case, the reaction from Step 2 is already balanced.
Combustion Reactions
Determine
the fuel (the source of carbon and/or hydrogen) and the oxidant (the source of
oxygen) (see Resources). If the combustion is carried out in air, the oxidant
is assumed to be molecular oxygen (O?). Other oxidants, such as nitrous oxide
(N?O), are possible, but this would require special reaction conditions.
Predict the
products by assuming this general reaction:
Fuel +
oxidant ? CO? + H?O
For example,
propane (C?H?) combines with O? during combustion as:
C?H? + O? ?
CO? + H?O
Balance the
reaction. For the example in Step 2:
C?H? + 5 O?
? 3 CO? + 4 H?O
Predicting Reaction Products - Solutions
Balance the equations and predict the products for the
following reactions:
1) 3 Na + 1 FeBr3 3
NaBr + 1 Fe
2) 2 NaOH + 1 H2SO4
1 Na2SO4 + 2 H2O
3) 1 C2H4O2 + 2 O2
2 CO2 + 2 H2O
4) 1 NH3 + 1 H2O 1
NH4OH
•
STEPS FOR PREDICTING PRODUCTS
Classify the reaction based on the reactants
Classify the reaction based on the reactants
•
Predict the
products based on the type of reaction
•
Write the formula for each product (Take into
consideration type of bonds, polyatomic ions, & diatomic elements)
Balance the chemical equation and use the solubility table to add state
symbols
Diatomics!
• Remember the elements that exist in
diatomic form.
• H, N, O,
F, Cl, Br and I
• All exist
with two of the atoms bonded together:
• H2
N2 O2 F2
Cl2 , Br2 , I2
Polyatomic
Ions!
• MEMORIZE YOUR POLYATOMICS
– Ammonium NH4+1
– Hydroxide
OH-1
– Nitrite NO2-1
– Nitrate NO3-1
– Hydrogen
sulfate HSO4-1
– Hydrogen
carbonate (bicarbonate) HCO3 -1
– Carbonate
CO3-2
– Sulfate SO4-2
– Phosphate
PO4 -3
This comment has been removed by a blog administrator.
ReplyDeletewhat the mean Predict the products based on the type of reaction?
ReplyDeleteWhat are the advantages of polyatomic ions
ReplyDeletee tables below list common polyatomic ions that you will be using throughout this General-Chemistry laboratory series (Chem 151-152). These ions are separated by charge on the ion into four (4) different tables and listed alphabetically within each table. For each polyatomic ion, the name, chemical formula, two-dimensional drawing, and three-dimensional representation are given.
DeleteThe three-dimensional structures are drawn as CPK models. CPK structures represent the atoms as spheres, where the radius of the sphere is equal to the van der Waals radius of the atom; these structures give an approximate volume of the polyatomic ion. In these tables, the three-dimensional structures have all been drawn to the same scale; therefore you can compare their relative sizes. In addition, the atoms in the CPK structures have been color-coded to match the two-dimensional drawings for easier comparison.
The decomposition reaction involves a single compound which divides into two or more compounds give an example?
ReplyDeleteDecomposition is a type of chemical reaction. It is defined as the reaction in which a single compound splits into two or more simple substances under suitable conditions. It is just the opposite of the combination reaction.
DeleteIn a combination reaction, a substance is formed as a result of chemical combination, while in a decomposition reaction, the substance breaks into new substances.
For example: The digestion of food in our body is accompanied by a number of decomposition reactions. The major constituents of our food such as carbohydrates, fats, proteins, etc.,decompose to form a number of simpler substances. These substances further react, releasing large amounts of energy, which keeps our body working.
Please give an example of the displacement reaction
ReplyDeleteThe reaction between zinc metal and hydrochloric acid to produce zinc chloride and hydrogen gas is an example of a single displacement reaction:
DeleteZn(s) + 2 HCl(aq) → ZnCl2(aq) + H2(g)
Another example is the displacement of iron from an iron(II) oxide solution using coke as a carbon source:
2 Fe2O3 (s) + 3 C (s) → Fe(s) + CO2 (g)
Give more an example polyatomic ion?
ReplyDeleteMany ions are monoatomic, which means that they are composed of just one atom. However, ions can also be polyatomic, composed of a group of atoms.
DeleteFor example, take a look at the following table. Notice anything about the Mercury(I) ion? Its ion symbol, Hg22+, shows that two mercury atoms are bonded together. This group has a 2+ charge, with each mercury cation having a 1+ charge. The mercurous ion is classified as a polyatomic ion.
Explain what is meant by ionic and covalent compounds?
ReplyDeleten ionic bond is a chemical bond between two atoms in which one atom seems to donate its electron to another atom. Covalent bonds, on the other hand, appear to involve two atoms sharing electrons reach a more stable electron configuration. Some compounds contain both ionic and covalent bonds. These compounds contain polyatomic ions. Many of these compounds contain a metal, a nonmetal, and also hydrogen.
ReplyDelete