Balancing Chemical Equations
1 answer:
Start by assigning the most complicated species a coefficient of one. That species should contain the greatest number of elements, e.g. .
<em>(not balanced)</em>
Assign coefficients to the rest of the species based on the conservation of atoms. For instance, the left hand side of the equation now contains one atom of hydrogen H and one atoms of chlorine Cl. The left hand side shall have an identical configuration. Both zinc chloride and hydrogen
should therefore have a coefficient of 1/2. (Don't panic about the fractions. They are to be eliminated in a few more steps.)
<em>(not balanced)</em>
The coefficient 1/2 in front of zinc chloride indicates the presence of 1/2 zinc atom in the right hand side of the equation. Zinc on the left hand side of the equation should accordingly have a coefficient of 1/2.
Increasing coefficients on both sides of the equation by a factor of two to eliminate all fractions. Hence the balanced equation.
(balanced)
The same set of operations should work for the second equation.
(balanced)
Note that the third equation does not accurately represent the catalytic decomposition of hydrogen peroxide . The balanced equation should be:
(balanced)
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Answer: 1. : oxidation reduction
2. : precipitation
3. : Double displacement
Explanation:
Oxidation-reduction reaction or redox reaction is defined as the reaction in which oxidation and reduction reactions occur simultaneously.
Oxidation reaction is defined as the reaction in which a substance looses its electrons. The oxidation state of the substance increases.Reduction reaction is defined as the reaction in which a substance gains electrons. The oxidation state of the substance gets reduced.
Double displacement reaction is defined as the reaction where exchange of ions takes place. Double displacement reaction in which one of the product remain in solid form are represented by (s) after their chemical formulas. Such double displacement reaction are called as precipitation reaction.
Double displacement reaction is defined as the reaction where exchange of ions takes place.
Single displacement reaction is defined as the reaction where more reactive element displaces a less reactive element from its chemical reaction.
Decomposition reaction is defined as the reaction where a single substance breaks down into two or more simpler substances.
Synthesis/Combination reaction is defined as the reaction where substances combine in their elemental state to form a single compound.