CHEMICAL EQUATIONS: MORE WRITING AND BALANCING PRACTICE Go through this PowerPoint for extra tips...
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Transcript of CHEMICAL EQUATIONS: MORE WRITING AND BALANCING PRACTICE Go through this PowerPoint for extra tips...
CHEMICAL EQUATIONS:MORE WRITING AND
BALANCING PRACTICE
Go through this PowerPoint for extra tips and extra practice!
CHEMICAL EQUATIONS Two basic rules apply in writing chemical equations:
We cannot write an equation for a reaction unless we know how the substances react and what new substances they form
Every chemical equation must be balanced (the number of atoms of each element on the left side must be the same as the number of atoms of that element on the right side of the equation)
Chemical equations are balanced according to the law of conservation of mass
nothing is created from nowhere or destroyed to nowhere.
Mass of matter present after the reaction is the same as before the reaction
A rearrangement of entities at the molecular level has occurred
COMMUNICATING CHEMICAL REACTIONS
Chemical Equations from Word Equations
Hydrogen gas burns in the presence of oxygen gas to produce water vapour
H2(g) + O2(g) H2O(g) (unbalanced)
2H2(g) + O2(g) 2H2O(g) (balanced)
Sodium metal reacts with chlorine gas to form sodium chloride
Na(s) + Cl2(g) NaCl(s)(unbalanced)
2Na(s) + Cl2(g) 2NaCl(s) (balanced)
A solution of silver nitrate reacts with a solution of potassium chloride to form a precipitate of silver chloride and a solution of potassium nitrate
AgNO3(aq) + KCl(aq) AgCl(s) + KNO3(aq)
COMMUNICATING CHEMICAL REACTIONS
Word Equations from Chemical Equations
NaOH(aq) + HCl(aq) NaCl(aq) + H2O(l)
A sodium hydroxide solution and a hydrochloric acid solution will react to produce a solution of sodium chloride and liquid water
2Na(s) + 2H2O(l) H2(g) + 2NaOH(aq)
Solid sodium metal and water will react to produce hydrogen gas and a solution of sodium hydroxide
C(s) + O2(g) CO2(g)
Solid carbon and oxygen gas will react (burn) to produce carbon dioxide gas
CaCO3(s) CaO(s) + CO2(g)
Solid calcium carbonate (when heated) will decompose to form solid calcium oxide and carbon dioxide gas
PRACTICE
Rewrite the following word equations as formula equation and balance them:
a) Solid potassium metal reacts with oxygen gas to produce solid potassium oxide
b) Methane gas reacts with oxygen gas to produce carbon dioxide gas and water vapour
c) Mercury(II) sulfide is decomposed into liquid mercury and solid sulfur
d) Aqueous cobalt(III) nitrate reacts with solid zinc to produce aqueous zinc nitrate and solid cobalt.
PRACTICE Answers: (remember: when there is no coefficient in front of a compound, there
is an invisible “1” there)
a) Solid potassium metal reacts with oxygen gas to produce solid potassium oxide
4K(s) + O2(g) 2K2O(s)
b) Methane gas reacts with oxygen gas to produce carbon dioxide gas and water vapour
CH4(g) + 2O2(g) CO2(g) + 2H2O(g)
c) Mercury(II) sulfide is decomposed into liquid mercury and solid sulfur
8HgS(s) 8Hg(l) + S8(s)
d) Aqueous cobalt(III) nitrate reacts with solid zinc to produce aqueous zinc nitrate and solid cobalt
2Co(NO3)3(aq) + 3Zn(s) 3Zn(NO3)2(aq) + 2Co(s)
CHEMICAL EQUATIONS A balanced chemical equation has the total atoms/ions on reactant side equal to the total number of the same kind of atom/ions on the product side
Coefficients are used as necessary in front of the chemical formulas of the skeletal equation to produce a balanced equation
States of matter are provide after each chemical formula
Summary and Practice on Pages 49 – 50 of Text
BALANCING CHEMICAL REACTION EQUATIONS
General steps for balancing chemical equations
Write an equation using the correct chemical formulas
Check the formulas of the reactants and products
Determine if the equation is balanced
Count the number of atoms of each element on the left side and the right side. Count polyatomic ion as a group if its formula is unchanged
Balance the equation one element at a time
Pick an element and balance the equation for that element by placing coefficients in front of the formulas to equalize the number of that element on both sides of the equation
A typical starting point is with the most complex formula
Balance diatomic elements last
Check to see if the equation is balanced
Sometimes balancing one element will put another element out of balance. If that happens, repeat steps 3 and 4 until the equation is balanced. Make sure the coefficients you use are the smallest possible whole numbers.
Never try to balance an equation by changing the subscripts in a formula – that would make the formula incorrect!
EXAMPLES
Balance the following chemical equations
Note: if polyatomic ions appear on both sides, keep them as a whole thing
Also it might be easier to write water as HOH instead of H2O if
hydroxide ions () are present on the other side of the equation
Note: fractions are not used for balancing equations – get rid of them by multiplying all coefficients in the equation by the denominator of the fraction
EXAMPLES
Answers:
1. 3Note: if polyatomic ions appear on both sides, keep them as a whole thing
Also it might be easier to write water as HOH instead of H2O if
hydroxide ions () are present on the other side of the equation
Note: fractions are not used for balancing equations – get rid of them by multiplying all coefficients in the equation by the denominator of the fraction
DO NOT
change correct chemical formulas and/or subscripts to make atoms of an element balance
add some real or imaginary chemical species to either side of the equation just to make atoms of an element balance
DO
perform a check to make sure all atoms/ions balance most chemical equations are balanced by what is called the inspection
method
This is somewhat a trial and error method which succeeds in most instances
Practice is necessary to become successful
Useful strategies develop as practice continues.
PRACTICE
Balance the following chemical equations
1. __Na(s) + __O2(g) __Na2O(s)
2. __HI(g) __H2(g) + __I2(g)
3. __SnF4(aq) + __Cr(s) __CrF3(aq) + __Sn(s)
4. __(NH4)3PO4(aq) + __CaBr2(aq) __Ca3(PO4)2(s) + __NH4Br(aq)
5. __C3H8(g) + __O2(g) __CO2(g) + __H2O(g)
6. __Al(NO3)3(aq) + __NaOH(aq) __NaNO3(aq) + __Al(OH)3(s)
PRACTICE
Answers: (Remember: it is not necessary to write down the coefficient when it is “1,” I put
it here to make it easier to understand. It is more conventionally correct to NOT put it.)
1. 4Na(s) + 1O2(g) 2Na2O(s)
2. 2HI(g) 1H2(g) + 1I2(g)
3. 3SnF4(aq) + 4Cr(s) 4CrF3(aq) + 3Sn(s)
4. 2(NH4)3PO4(aq) + 3CaBr2(aq) 1Ca3(PO4)2(s) + 6NH4Br(aq)
5. 1C3H8(g) + 5O2(g) 3CO2(g) + 4H2O(g)
6. 1Al(NO3)3(aq) + 3NaOH(aq) 3NaNO3(aq) + 1Al(OH)3(s)