Chem 1010 - General Chemistry 1 » Fall 2021 » CH3 Chemical Reactions
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Question #1
Which of these equations is not balanced?
A.
C6H6(l) + O2(g) → H2O(l) + CO2(g)
B.
2 H3BO3(s) → B2O3(s) + 3 H2O(l)
C.
B2O3(s) + 6 HF(aq) → 2 BF3(l) + 3 H2O(l)
D.
3 MgO(s) + 2 Fe(s) → Fe2O3(s) + 3 Mg(s)
Question #2
Choose the balanced equation
A.
N2(g) + 3 H2(g) → 2 NH3(g)
B.
H3BO3(s) → B2O3(s) + H2O(l)
C.
Fe(s) + H2O(g) → Fe3O4(s) + H2(g)
D.
Fe(s) + Cl2(g) → FeCl3(s)
Question #3
Which shows the balanced reaction between iron(III) oxide and aluminum?
A.
2 Al(s) + Fe2O3(s) → Al2O3(s) + 2 Fe(s)
B.
Al(s) + FeO2(s) → AlO3(s) + Fe(s)
C.
Al(s) + Fe2O3(s) → AlO3(s) + Fe(s)
D.
Al(s) + Fe2O3(s) → Al3O2(s) + Fe(s)
Question #4
Which of these equations is the balanced reaction between sulfurous acid and magnesium hydroxide?
A.
H2S(g) + MgOH(s) → MgS(s) + H2O(l)
B.
H2SO3(l) + MgOH(s) → MgSO4(s) + 2 H2O(l)
C.
H2SO3(l) + Mg(OH)2(s) → MgSO3(s) + 2 H2O(l)
D.
H2SO4(l) + Mg(OH)2(s) → MgSO4(s) + 2 H2O(l)
Question #5
Which of these compounds is insoluble in water?
A.
KClO3
B.
AgCl
C.
MgCl2
D.
(NH4)2S
Question #6
Which anions form compounds that are usually soluble?
A.
Nitrates
B.
Hydroxides
C.
Phosphates
D.
Carbonates
Question #7
Which of these species is a strong acid?
A.
HCl
B.
Cl-
C.
H2NCH2CH3
D.
H2CO3
Question #8
What is the oxidation number of phosphorus in PO33- ?
A.
+7
B.
+5
C.
+1
D.
+3
Question #9
Which of these species can serve as a common reducing agent?
A.
H2O2
B.
Cr2O72-
C.
F2
D.
Fe
Question #10
Benzoic acid (C6H5COOH) and ethanol (CH3CH2OH) react according to this equation to produce C6H5COOCH2CH3: C6H5COOH(s) + CH3CH2OH(l) → C6H5COOCH2CH3(s) + H2O(l) If 15.6 g C6H5COOH and 11.9 g CH3CH2OH are reacted, how many grams of C6H5COOCH2CH3 are produced?
A.
50.9 g
B.
19.2 g
C.
38.8 g
D.
12.7 g
Question #11
How many grams of nickel(II) nitrate are needed to produce 35.9 g nickel(II) phosphate in the presence of excess sodium phosphate?
A.
91.0 g nickel(II) nitrate
B.
28.2 g nickel(II) nitrate
C.
17.9 g nickel(II) nitrate
D.
53.8 g nickel(II) nitrate
Question #12
How many moles of iron(III) hydroxide are needed to react with excess nitric acid to produce 61.1 g iron(III) nitrate?
A.
0.315 mol
B.
0.253 mol
C.
0.758 mol
D.
0.572 mol
Question #13
Consider this reaction: CH3COOH(l) + CH3CH2OH(l) → CH3C(O)OC2H5(l) + H2O(l) The actual yield is 72.1 g CH3C(O)OC2H5 . If you start with 54.4 g CH3COOH, what is the percent yield of this reaction?
A.
55.3%
B.
111%
C.
90.4%
D.
75.4%
Question #14
The following reaction has a percent yield of 87.9%. How many grams of carbon dioxide are produced from 72.2 g calcium carbonate via this reaction? 2 HNO3(aq) + CaCO3(aq) → Ca(NO3)2(aq) + H2O(l) + CO2(g)
A.
31.7g
B.
36.1%
C.
19.9g
D.
27.9g
Question #15
A compound has a percent composition of 68.8% C, 4.92% H, and 26.2% O. Determine the empirical formula of this compound.
A.
C7H6O2
B.
C6H6O2
C.
C3H3O
D.
C4H3O
Question #16
Which equation shows the total molecular reaction between potassium carbonate and phosphoric acid?
A.
3 K+(aq) + PO43-(aq) → 2 K3PO3(aq)
B.
3 K2CO3(aq) + 2 H3PO4(aq) → 2 K3PO3(aq) + 3 CO2(g) + 3 H2O(l )
C.
CO3(aq) + 3 H+(aq) → 3 CO2(g) + 3 H2O(l )
D.
3 K 2 CO3(aq) + 2 H3PO4(aq) → 2 K3PO3(aq) + 3 H2CO3(aq)
Question #17
Which species is being reduced in this reaction? SnO2(s) + C(s) Sn(s) + CO2(g)
A.
SnO2
B.
CO2
C.
Sn
D.
C
Question #18
A.
0.823 M
B.
0.000161 M
C.
0.161 M
D.
0.0329 M
Question #19
Calculate the number of milliliters of 0.764 M KOH needed to make 250 mL of a 0.120 M KOH solution.
A.
2.29 mL
B.
0.0393 mL
C.
3.93 mL
D.
39.3 mL
Question #20
How many grams of barium sulfate will precipitate when 15.0 mL of 0.354 M barium chloride is mixed with 15.0 mL of 0.307 M sodium sulfate?
A.
1.07 g
B.
0.54 g
C.
1.24 g
D.
2.31 g
Question #21
A.
2 H+(aq) + 2 Cl-(aq) +Ca(OH)2(s) → Ca2+(aq) + 2 Cl-(aq) + 2 H2O(l)
B.
H+(aq) + OH-(aq) → H2O(l)
C.
2 HCl(aq) + Ca(OH)2(s) → CaCl2(aq) + 2 H2O(l)
D.
2 H+(aq) + 2 Cl-(aq) + Ca2+(aq) + 2 OH-(aq) → Ca2+(aq) + 2 Cl-(aq) + 2 H2O(l)
Question #22
You are given 0.8575 g of an unknown diprotic acid, H2A. It reacts with NaOH according to this balanced equation: H2A(aq) + 2 NaOH(aq) Na2A(aq) + 2 H2O(l) If a volume of 34.35 mL of 0.5934 M NaOH is required to react with all of the acid, what is the molar mass of the acid?
A.
21.0 g/mol
B.
42.1 g/mol
C.
49.1 g/mol
D.
84.1 g/mol
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