Chapter 11 Test Review

Balance the following equation so that there are the same number of atoms on each side of the yield sign. Click on the answer box to reveal the answer. What numbers should be added to the equation, if any? Write them in the spaces below. __CaCO3 __CaO + __CO2 Answer CaCO3 CaO + CO2

__C + __Cl2 __CCl4 Balance the following equation. Answer

__NaH2PO4 __NaPO3 + ___H2O Balance the following equation. Answer 1, 1, 1

__H2 + __Cl2 __HCl Balance the following equation. Answer

Balance the following equation. __Na + __F2 __NaF Answer 2Na + F2 2NaF

__H2O2 __H2O + __O2 Balance the following equation. Answer

__KClO3 __KCl + __O2 Balance the following equation. Answer

__P + __O2 __P4O10 Balance the following equation. Answer

___KMnO4 + ___HCl ___KCl + ___MnCl2 + ___H2O + ___Cl2 Balance the following equation. ___KCl + ___MnCl2 + ___H2O + ___Cl2 ___KMnO4 + ___HCl Answer 2,16 2,2,8,5

___H2SO4 + ___V2O3 ___V2(SO4)3 + ___H2O Balance the following equation. ___H2SO4 + ___V2O3 ___V2(SO4)3 + ___H2O Answer 3,1 1,3

___SO2 + ___H2O ___H2S + ___O2 Balance the following equation. Answer 10,10 10,1

__BaCl2 + __H2SO4 __BaSO4 + __HCl Balance the following equation. __BaCl2 + __H2SO4 __BaSO4 + __HCl Answer BaCl2 + H2SO4 BaSO4 + 2HCl

Balance the following equation. __N2 + __H2 __NH3 Answer N2 + 3H2 2NH3

__Na + __Cl2 __NaCl Balance the following equation. Answer

Word Match the word with its definition. Definition reactant a representation of a chemical reaction showing the relative numbers of reactant and product molecules a number written before a chemical formula to represent the relative numbers of the molecule a substance resulting from a chemical reaction a process in which one or more substances are changed into one or more new substances by the reorganization of component atoms the starting substance in a chemical reaction reactant coefficient chemical equation chemical reaction product

The formula HCl stands for ____. hydrochloric acid

____ measures how acidic or basic a substance is. 2 ____ measures how acidic or basic a substance is. pH

3 What type of reaction is shown in the following chemical equation: 2H2O ® 2H2 + O2? decomposition

4 According to the law of conservation of mass, if two atoms of hydrogen are used as a reactant, how many atoms of hydrogen must be part of the product? 2

5 According to the law of conservation of mass, how does the mass of the products in a chemical reaction compare to the mass of the reactants? The masses are equal.

6 Numbers that precede symbols and formulas in a chemical equation are ____. coefficients

synthesis What type of reaction is shown in the following 7 What type of reaction is shown in the following chemical equation: NH3 + HCl ® NH4Cl? synthesis

Each substance on the left side of the arrow in a chemical equation is a ____. reactant

balanced A(n) ____ chemical equation has the same number of 9 A(n) ____ chemical equation has the same number of atoms of each element on each side of the equation. balanced

__Fe + __O2 __Fe2O3 Balance the following equation. Answer

Word Description Type of reaction where we have more products than reactants (numerically wise) Type of reaction where two things are added, giving us one product. Type of reaction where we need to use our metal activity series...only reaction where there can be no reaction. Type of reaction that characterizes burning. Most common type of chemical reaction. Synthesis Combustion Double Replacement Decomposition Single Replacement

Write this chemical equation in word form: Cu(s) + 2 H2O(l) Cu(OH)2(aq) + H2(g)

Write this chemical equation in word form: CO(g) + SO3 CO2(g) + SO2(g)

·Write the molecular, total ionic, and net ionic equations for this reaction: Silver nitrate reacts with Lead (II) Chloride in hot water. ·(Remember your (aq), (l), & (s) symbols because those can make a difference in the net ionic equation.)

Molecular Equation: 2AgNO3(aq) + PbCl2(aq) = 2AgCl + Pb(NO3)2 Total Ionic Equation: 2Ag(s) + 2NO3 (aq) + PbCl2(aq) = 2AgCl + Pb(s) + 2NO3 (aq) Net Ionic Equation: 2Ag(s) + PbCl2(aq) = 2AgCl + Pb(s)

Write the molecular, total ionic, and net ionic equations for this reaction: CaCO3(s) + HCl One of the the products in this is H2CO3 which then decomposes to CO2 and liquid water...use these two products in your equations.

Molecular Equation: CaCO3(s) + 2HCl(aq) = CaCl2(aq) + H2O(l) + CO2(g) Total Ionic Equation: CaCO3(s) + 2H+(aq) + 2Cl-(aq) = Ca2+(aq) + 2Cl-(aq) + H2O(l) + CO2(g) Net Ionic Equation: CaCO3(s) + 2H+(aq) = Ca2+(aq) + H2O(l) + CO2(g)

Write the molecular, total ionic, and net ionic equations for this reaction: Fe(s) + AgNO3

Molecular Equation: Fe(s) + 2AgNO3(aq) = 2Ag(s) + Fe(NO3)2(aq) Total Ionic Equation: Fe(s) + 2Ag+(aq) + 2NO3-(aq) = 2Ag(s) + Fe2+(aq) + 2NO3-(aq) Net Ionic Equation: Fe(s) + 2Ag+(aq) = 2Ag(s) + Fe2+(aq)

What type of reaction is the following: H2 + O2

What type of reaction is the following: KBr + Cl2

What type of reaction is the following: Zn + H2SO4

What type of reaction is the following: C4H10 + O2

What type of reaction is the following: HgO

What type of reaction is the following: AgNO3 + NaCl

What type of reaction is the following: C8H8 + O2

What type of reaction is the following: Mg(OH)2 + H2SO3