Match the type of chemical reaction with the appropriate skeleton equation.
Answer
A.
Single Replacement
B.
Decomposition
C.
Synthesis
D.
Combustion
E.
Double Replacement
QUESTION 1
Balanced chemical equations show:
the reactants entering the reaction
the products formed by the reaction
the ratios of moles needed to balance the reactants and products
all of the above
3 points Save Answer
QUESTION 2
In the equation, CaCO3 (s) Imported Asset CaO (s) + CO2 (g), the mass of the reactants:
is greater than the mass of the products because a gas is released on the product side of the equation
is less than the mass of the products because the mass of the gas is not included on the reactant side of the equation
is the same as the mass of the products
has no relationship to the mass of the products
3 points Save Answer
QUESTION 3
When balancing a chemical equation, where should a coefficient be placed?
in front of formulas and element symbols
in front of individual elements and behind individual compounds
behind formulas and element symbols
by the lower right hand corner of element or compound formulas, to indicate numbers of atoms
3 points Save Answer
QUESTION 4
Coefficients should always:
be whole numbers
use the lowest possible ratios
use the values of 1, 2, 3, or 4
both choices a and b
3 points Save Answer
QUESTION 5
What is the molar ratio for the following equation after it has been properly balanced?
____SiO2 + ____C Imported Asset ____ SiC + ____CO
Reactants: SiO2 = 1, C = 3; Products: SiC = 1, CO = 2
Reactants: SiO2 = 1, C = 2; Products: SiC = 1, CO = 2
Reactants: SiO2 = 2, C = 3; Products: SiC = 2, CO = 2
Reactants: SiO2 = 3, C = 3; Products: SiC = 3, CO = 2
3 points Save Answer
QUESTION 6
What is the molar ratio for the following equation after it has been properly balanced?
____C3H8 + ____O2 Imported Asset ____CO2 + ____ H2O
Reactants: C3H8 = 2, O2 = 5; Products: CO2 = 6 and H2O = 4
Reactants: C3H8 = 1, O2 = 5; Products: CO2 = 3 and H2O = 4
Reactants: C3H8 = 1, O2 = 8; Products: CO2 = 3 and H2O = 4
Reactants: C3H8 = 1, O2 = 5; Products: CO2 = 3 and H2O = 5
3 points Save Answer
QUESTION 7
What is the atom inventory for the following equation after it has been properly balanced?
____Li + ____BaF2 Imported Asset ____LiF + ____Ba
Reactants: Li = 2, Ba = 1, F = 2; Products: Li = 2, Ba = 1, F = 1
Reactants: Li = 1, Ba = 2, F = 2; Products: Li = 1, Ba = 2, F = 2
Reactants: Li = 2, Ba = 1, F = 2; Products: Li = 2, Ba = 1, F = 2
Reactants: Li = 1, Ba = 1, F = 2; Products: Li = 1, Ba = 1, F = 2
3 points Save Answer
QUESTION 8
If the combined mass of the reactants is 100 grams, then which of the following MUST be true?
the combined mass of the products is 100 grams
each product has a mass of 100 grams
each reactant has the same mass as each product
each reactant must produce 100 grams of product
3 points Save Answer
QUESTION 9
In the equation, A + B Imported Asset C + D, if the sum of the masses of reactants A and B is known, and the mass of product C is known, then the mass of product D can be calculated.
TRUE
FALSE
2 points Save Answer
QUESTION 10
Every chemical compound has a formula, which cannot be altered when balancing chemical equations.
TRUE
FALSE
2 points Save Answer
QUESTION 11
A balanced chemical equation must account for every atom involved in a chemical reaction.
TRUE
FALSE
Given the reaction, PCl3 + Cl2 Imported Asset PCl5, if 3.00 moles of Cl2 are used, then how many moles of PCl5 are made?6.00 moles5.00 moles3.00 moles1.00 mole3 points Save AnswerQUESTION 2Given the balanced equation, 2 SO2 + O2 Imported Asset 2 SO3, what is the molar ratio of O2 to SO3?2:11:22:22:33 points Save AnswerQUESTION 3Given the balanced equation, 4 NH3 + 3 O2 Imported Asset 2 N2 + 6 H2O, what is the molar ratio of NH3 to N2?3:24:62:44:23 points Save AnswerQUESTION 4Using the equation, C5H12 + 8O2 Imported Asset 5CO2 + 6H2O, if an excess of pentane (C5H12) were supplied, but only 4 moles of oxygen were available, how many moles of water would be produced?1 mole2 moles3 moles6 moles3 points Save AnswerQUESTION 5Using the equation, C5H12 + 8O2 Imported Asset 5CO2 + 6H2O, if 10 moles of carbon dioxide are produced, how many moles of pentane (C5H12) would need to be supplied?2 moles0.5 mole5 moles10 moles3 points Save AnswerQUESTION 6Using the equation, 4Fe + 3O2 Imported Asset 2Fe2O3, if 8 moles of iron and oxygen from the air were available, how many moles of iron (III) oxide would be produced?4 moles5 moles6 moles8 moles3 points Save AnswerQUESTION 7When magnesium metal and an aqueous solution of hydrochloric acid combine, they produce an aqueous solution of magnesium chloride and hydrogen gas. Using the equation, Mg (s) + 2HCl (aq) Imported Asset MgCl2 (aq) + H2 (g), if 72.9 g of Mg and 146.0 g of HCl are allowed to react, identify the limiting reagent.MgHClMgCl2H23 points Save AnswerQUESTION 8When magnesium metal and an aqueous solution of hydrochloric acid combine, they produce an aqueous solution of magnesium chloride and hydrogen gas. Using the equation, Mg (s) + 2HCl (aq) Imported Asset MgCl2 (aq) + H2 (g), if 24.3 g of Mg and 75.0 g of HCl are allowed to react, calculate the mass of MgCl2 that is produced.75.0 g95.1 g99.3 g104 g3 points Save AnswerQUESTION 9The number of moles of the reagent in excess can be used to calculate the moles of the products of the reaction.TRUEFALSE2 points Save AnswerQUESTION 10In the manufacturing process of sulfuric acid, sulfur dioxide is reacted with oxygen to produce sulfur trioxide. Using the equation, 2SO2 (g) + O2 Imported Asset 2SO3 (g), if 64.06g of sulfur dioxide is given an opportunity to react with an excess of oxygen to produce 75.00 g of sulfur trioxide, what is the percent yield of this reaction?46.83%60.25%75.55%93.68%3 points Save AnswerQUESTION 11Red mercury (II) oxide decomposes to form mercury metal and oxygen gas according to the following equation: 2HgO (s) Imported Asset 2Hg (l) + O2 (g). If 3.00 moles of HgO decompose to form 1.25 moles of O2 and 503 g of Hg, what is the percent yield of this reaction?41.6%62.5%83.3%96.9%3 points Save AnswerQUESTION 12Red mercury (II) oxide decomposes to form mercury metal and oxygen gas according to the following equation: 2HgO (s) Imported Asset 2Hg (l) + O2 (g). If 4.00 moles of HgO decompose to form 1.50 moles of O2 and 603 g of Hg, what is the percent yield of this reaction?26.7%53.4%75.0%95.5%3 points Save AnswerQUESTION 13The percent yield for a chemical reaction can not be calculated until the reaction is completed.TRUEFALSE2 points Save AnswerQUESTION 14The theoretical yield for a chemical reaction can not be calculated until the reaction is completed.TRUEFALSE