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Specific Reactions Quiz
Name:
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Knowledge. Answer the following questions on foolscap.
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1. What are all the necessary conditions for a combustion that is complete?
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2. Consider each of the following characteristics of incomplete combustion. Explain the reason for each characteristic.
a) the production of soot
b) a lingering flame
c) a quiet explosion or pop
d) a chemical equation which cannot be balanced
e) less than optimum amounts of energy
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3. Explain the overall general process of acids/base production that is similar or common to both.
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4. Predict whether the product of the following reactions will be an acid, a base or neutral.
a) H2O(l) + Hg(s) ö
d) pure phosphorus burned in air and then dissolved into water ö
b) H2O(l) + MgO(s) ö e) Ba(s) + H2O(l) ö
c) Cl2O(s) + H2O(l) ö f) K(s) + O2(g) ö product + H2O(l) ö
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5.a) Explain how water is more than just a solvent in acid preparation using an oxide.
b) Explain how water is more than just a solvent in base preparation using an oxide.
c) Identify one factor which affects how acidic/basic a solution becomes as a result of these oxide
reactions (aside from amount of oxide use).
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6. Write the balanced chemical equation for each of the following acid/base reactions:
a) Ca(OH)2(aq) + H3PO4(aq) ö
c) H2SO4(aq) + BaCO3(aq) ö
b) CH3COOH(aq) + Ag2SO3(aq) ö
d) Fe(s) + HNO3(aq) ö
Sodium
Barium
Calcium
Magnesium
Aluminum
Zinc
Nickel
Lead
Hydrogen
Copper
Silver
Mercury
Gold
Specific Reactions Quiz
Name:
/33
Knowledge. Answer the following questions on foolscap.
/4
1. What are all the necessary conditions for a combustion that is complete?
!
!
!
!
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there needs to be an ignition source (to destabilize the fuel)
there must be sufficient oxygen for the amount of fuel
there must be sufficient mixing of the oxygen with the fuel
there must be a way to prevent the build up or accumulation of waste gases
2. Consider each of the following characteristics of incomplete combustion. Explain the reason for each characteristic.
a) the production of soot
b) a lingering flame
c) a quiet explosion or pop
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!
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a) various carbon products created due to lack of oxygen including solid carbon (black component)
b) as air contacts the random carbon products (smaller hydrocarbons) created, they may further
combust
c) since energy is still tied up in carbon product bonds, energy is not released all at once
d) the presence of random carbon products prevents balancing
e) energy is lost because it remains trapped within any remnant fuel bonds
3. Explain the overall general process of acids/base production that is similar or common to both.
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!
!
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d) a chemical equation which cannot be balanced
e) less than optimum amounts of energy
something needs to split water
into H+ and OH–
but one of these ions needs to be changed or prevented from persisting
4. Predict whether the product of the following reactions will be an acid, a base or neutral.
a) H2O(l) + Hg(s) ö
d) pure phosphorus burned in air and then dissolved into water ö
b) H2O(l) + MgO(s) ö e) Ba(s) + H2O(l) ö
c) Cl2O(s) + H2O(l) ö f) K(s) + O2(g) ö product + H2O(l) ö
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c) acid
d) acid
e) base
f) base
an non-metal oxide bonds with the water
in a synthesis reaction
resulting in the production of a new chemical, a soluble oxyacid
b) Explain how water is more than just a solvent in base preparation using an oxide.
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!
!
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b) base
5.a) Explain how water is more than just a solvent in acid preparation using an oxide.
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!
!
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a) neutral
Sodium
Barium
Calcium
Magnesium
Aluminum
Zinc
Nickel
Lead
Hydrogen
Copper
Silver
Mercury
Gold
after the metal oxide dissolves into water creating O2–(aq)
O2–(aq) then breaks water down into H+(aq) and OH–(aq)
following which O2–(aq) combines with H+(aq) to become OH–(aq)
c) Identify one factor which affects how acidic/basic a solution becomes as a result of these oxide reactions (aside
from amount of oxide use).
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or
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solubility of the oxide compound (more soluble = more acidic/basic)
activity level of the non-metal/metal component of the oxide (more reactive the non-metal or metal
component of the oxide = more acidic/basic)
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6. Write the balanced chemical equation for each of the following acid/base reactions:
a) Ca(OH)2(aq) + H3PO4(aq) ö
c) H2SO4(aq) + BaCO3(aq) ö
b) CH3COOH(aq) + Ag2SO3(aq) ö
d) Fe(s) + HNO3(aq) ö
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a) 3 Ca(OH)2(aq) + 2 H3PO4(aq) ö Ca3(PO4)2(s) + 6 H2O(l)
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b) 2 CH3COOH(aq) + Ag2SO3(aq) ö 2AgCH3COO(s) + H2SO3(aq)
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c) H2SO4(aq) + BaCO3(aq) ö H2O(l) + CO2(g) + BaSO4(s)
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d) Fe(s) + 2 HNO3(aq) ö H2(g) + Fe(NO3)2(aq)
or
2 Fe(s) + 6 HNO3(aq) ö 3 H2(g) + 2 Fe(NO3)3(aq)
Prepared by K. Zuber