Chem 101 - General Chemistry I » Spring 2021 » Chapter 4 Homework Quiz
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Question #1
When the following equation is balanced using the smallest possible integers, what will be the coefficient for oxygen gas C3H8(g) + O2(g) → CO2(g) + H2O(g)
A.
7
B.
5
C.
3
D.
9
Question #2
When the following equations are balanced using the smallest possible integers, what will be the coefficient of the underlined substance in each case? C4H10(g) + O2(g) → CO2(g) + H2O(g)
A.
4
B.
6
C.
10
D.
8
Question #3
When the following equation is balanced using the smallest possible integers, what will be the coefficient for the substance that has been emboldened? CH3OH + O2 → CO2 + H2O
A.
1
B.
4
C.
3
D.
2
Question #4
When a precipitation reaction occurs, the ions that do not form the precipitate
A.
are cations only
B.
are left dissolved in the solution
C.
form a second insoluble compound in the solution
D.
none of these
Question #5
Which of the following ionic compounds is soluble in water?
A.
MgCO3
B.
CaCO3
C.
(NH4)2CO3
D.
Al2(CO3)3
Question #6
Which of the following ionic compounds is soluble in water?
A.
Cu3PO4
B.
Mg3(PO4)2
C.
AlPO4
D.
Na3PO4
Question #7
An aqueous solution of ammonium sulfate is allowed to react with an aqueous solution of lead(II) nitrate. What is the coefficient of the solid in the balanced equation (in standard form)?
A.
6
B.
4
C.
1
D.
3
Question #8
For the following reaction: H2PO3(aq)+2KOH(aq)⟶K2PO3(aq)+2H2O(l)H2PO3(aq)+2KOH(aq)⟶K2PO3(aq)+2H2O(l) Please write out the complete and net ionic equations. What is the coefficient for hydroxide ion in the complete ionic equation (input 0 if the hydroxide ion does not appear in the complete ionic equation):
A.
4
B.
2
C.
3
D.
5
Question #9
An aqueous solution of ammonium sulfate is mixed with an aqueous solution of barium nitrate. Which of the following species does the net ionic equation contain?
A.
2SO42-(aq)
B.
NO3-(aq)
C.
2NH4+(aq)
D.
Ba2+(aq)
Question #10
Which of the following is a conjugate acid–base pair?
A.
HNO3–, H2NO3
B.
At most one of the adults has high blood pressure.
C.
H2F, HF–
D.
HPO42–, PO43–
E.
H2CN, CN–
Question #11
True or false? Aluminum resists corrosion in air because aluminum metal gains electrons rather than losing electrons.
A.
TRUE
B.
FALSE
Question #12
The oxidation state of oxygen in O2 is
A.
–1
B.
–2
C.
+4
D.
0
E.
–4
Question #13
The oxidation state of chlorine in Cl2 is
A.
0
B.
none of these
C.
–2
D.
–1
E.
+1
Question #14
The oxidation state of manganese in MnO-4 is
A.
0
B.
+4
C.
+3
D.
+7
E.
+8
Question #15
Answer the questions that refer to the following reaction: TiCl4(l) + O2(g) → TiO2(s) + 2Cl2(g) Which species is oxidized?
A.
TiO2
B.
O
C.
Cl
D.
Ti
Question #16
Answer the questions that refer to the following reaction: SiO2(s) + 2C(s) → Si(s) + 2CO(g) Which species is the oxidizing agent?
A.
C
B.
CO
C.
O
D.
SiO2
Question #17
For the reaction of sodium bromide with chlorine gas to form sodium chloride and bromine, the appropriation half-reactions are (ox = oxidation and re = reduction)
A.
ox: 2Br– → Br2 + 2e– re: Cl2 + 2e– → 2Cl–
B.
ox: Br + 2e– → Br– re: 2Cl– → Cl2 + 2e–
C.
ox: Cl2 + 2e– → 2Cl– re: 2Br– → Br2 + 2e–
D.
ox: 2Na+ + 2e– → 2Na re: 2Cl– → Cl2 + 2e–
Question #18
How many electrons are transferred in the reaction, Ni + 2HCl → NiCl2 + H2?
A.
0
B.
4
C.
1
D.
2
Question #19
Balance the following oxidation–reduction reaction using the half-reaction method. Cr2O72– + I2 → Cr3+ + IO3– In the balanced equation, the coefficient of water is:
A.
17
B.
11
C.
4
D.
6
Question #20
When the following reaction is balanced in basic solution, what is the coefficient of thalium (III) oxide? Tl2O3+NH2OH⟶TlOH+N2Tl2O3+NH2OH⟶TlOH+N2
A.
1
B.
3
C.
4
D.
2
Question #21
The equation N2(g) + 3H2(g) → 2NH3(g) can be interpreted as follows: 1 mol of N2 reacts with 3 mol of H2 to form 2 mol of NH3. Is this statement true or false?
A.
TRUE
B.
FALSE
Question #22
A 3.8-mol sample of KClO3 was decomposed according to the equation 2KCl03(s) —> 2KCl(s) + 3O2(g) How many moles of O2 are formed assuming 100% yield?
A.
2.5 mol
B.
1.9 mol
C.
3.8 mol
D.
5.7 mol
E.
3.2 mol
Question #23
How many moles of oxygen are required for the complete reaction of 23.6 g of ethene to form carbon dioxide and water?
A.
0.421 mol
B.
1.68 mol
C.
3.37 mol
D.
2.52 mol
Question #24
Which of the following statements is always true concerning a reaction represented by the balanced chemical equation below? 2C2H6(g) + 7O2(g) → 4C02(g) + 6H20(g)
A.
If we have an equal number of moles of ethane and oxygen, there is no limiting reactant.
B.
If we have extra mass of ethane, then oxygen must be the limiting reactant.
C.
If we have extra mass of oxygen, then ethane must be the limiting reactant.
D.
If we have equal masses of ethane and oxygen, there is no limiting reactant.
E.
None of these statements are true.
Question #25
Look at the reaction below: Al(OH)3 + 3HC1 —> 3H20+ AlCl3 Suppose 0.55 g of water were produced from 1.2 g of aluminum hydroxide and a certain amount of hydrochloric acid. Which of the following statements is true? Choose the best answer.
A.
Aluminum hydroxide is not the limiting reactant because some amount of aluminum hydroxide is left.
B.
Aluminum hydroxide is the limiting reactant because 1.2 g of aluminum hydroxide produces 0.55 g of water.
C.
Aluminum hydroxide is not the limiting reactant because more than 0.55 g of water could have been produced from 1.2 g of aluminum hydroxide.
D.
Aluminum hydroxide is the limiting reactant because it has a smaller coefficient than hydrochloric acid.
Question #26
Consider the reaction of magnesium metal with hydrochloric acid to produce magnesium chloride and hydrogen gas. If 3.75 mol of magnesium and 3.75 mol of hydrochloric acid are reacted, how many grams of excess reactant are left over?
A.
45.6 g
B.
68.4 g
C.
1.88 g
D.
91.2 g
Question #27
In the reaction 2Al(s) + 3I2(s) → 2AlI3(s), the theoretical yield of the product is 12 g. When a student performed this reaction in his lab, he could obtain just 3 g of the product. Calculate the percent yield.
A.
25%
B.
30%
C.
20%
D.
40%
Question #28
When 38.4 g of CH4 reacts completely with excess chlorine yielding 45.0 g of CH3Cl, what is the percentage yield, according to CH4(g) + Cl2(g) → CH3Cl(g) + HCl(g)
A.
85.3
B.
14.7
C.
37.1
D.
121.2
Question #29
Tetraphosphorous hexaoxide is formed by the reaction of phosphorous (P4) with oxygen gas. If the reaction of 68.8 g of P4 with 18.8 g of O2 produces 21.0 g of P4O6, calculate the percent yield for the reaction.
A.
8280%
B.
17.2
C.
43.1
D.
48.7
Question #30
15.0 mL of 0.30 M sodium phosphate solution reacts with 20.0 mL of 0.20 M lead(II) nitrate solution. What mass of precipitate will form?
A.
3.2 g
B.
3.1 g
C.
1.1 g
D.
1.8 g
Question #31
In the following acid-base neutralization, 1.31 g of the solid acid HC6H5O neutralized 11.61 mL of aqueous NaOH solution base by the reaction NaOH(aq) + HC6H5O(aq) → H2O(l) + NaC6H5O(aq) Calculate the molarity of the base solution.
A.
0.113 M
B.
0.162 M
C.
1.20 M
D.
8.86 M
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