Not to be confused with "proselytizing"
What is the maximum possible quantity of product obtained from a chemical reaction called?
A) Percent yield
B) molecular weight of the product
C) stoichiometric coefficients
D) limiting reagent
E) theoretical yield
E) theoretical yield
If 225 g of pure carbon (12.01 g/mol) in an experiment reacts with excess sulfur dioxide to produce 195 g of carbon disulfide (76.15 g/mol), what is the percent yield for the reaction?
5 C + 2 SO2 -> CS2 + 4 CO
A) 78.9%
B) 68.4%
C) 22.5%
D) 19.5%
E) 15.7%
B) 68.4%
Which of the following ionic compounds is insoluble in water?
A) FeCl3
B) NH4CH3COO
C) AgNO3
D) K2CO3
E) Cu2(PO4)2
E) Cu2(PO4)2
What is the oxidation number of bromine in NaBrO2?
A) -1
B) +1
C) +3
D) +5
E) -3
C) +3
Lycopene, a red pigment found in tomatoes has the empirical formula C5H7 and its molar mass is approximately 536.888 g/mol. Which of the following is the correct molecular formula?
A. C5H7
B) C15H21
C) C30H42
D) C40H56
E) C50H70
D) C40H56
How many grams of TiCl4 (189.9 g/mol) are needed to produce 0.132 moles of MgCl2 in the given unbalanced reaction?
Mg + TiCl4 -> Ti + MgCl2
A) 6.26 g
B) 25.0 g
C) 12.5 g
D) 50.1 g
E) 24.4 g
C) 12.5 g
DAILY DOUBLE
Solid aluminum reacts with gaseous chlorine gas to make aluminum chloride according to the balanced equation below. If a reaction is ran with 3.0 moles aluminum and 7.0 moles chlorine gas, the limited reactant is ____ and ____ moles of aluminum chloride could be formed.
2 Al (s) + 3 Cl2 (g) -> Al2Cl6 (s)
A) Al, 1.5 mol
B) Cl2, 1.5 mol
C) Al, 4.0 mol
D) Al, 2.5 mol
E) Cl2, 4.0 mol
A) Al, 1.5 mol
Aqueous magnesium acetate (Mg(CH3COO)2) and aqueous lithium hydroxide (LiOH) are mixed to produce aqueous lithium acetate and solid magnesium hydroxide. What are the spectator ions?
A) Mg2+ and CH3OO-
B) Li+ and OH-
C) Mg2+ and OH-
D) Li+ and CH3OO-
E) Li+, CH3OO- and Mg2+
D) Li+ and CH3OO-
In what compound does the iodine have an oxidation number of +3?
A) HIO4
B) HIO3
C) HIO2
D) HIO
E) HI
C) HIO2
Which of the following statements regarding weak acids is correct?
A) Solutions of weak acids have very low concentrations
B) Weak acids can be strong or weak electrolytes
C) The concentration of the molecule is greater than its ions when dissolved
D) Weak acids are always monoprotic acids
E) Nitric acid is an example
C) The concentration of the molecule is greater than its ions when dissolved
Calculate the molarity of a solution made by adding 126 g of NaNO3 (85.00 g/mol) to enough water to make 250.0 mL of solution
A) 0.371 M
B) 0.504 M
C) 5.93 M
D) 0.167 M
E) 4.28 M
C) 5.93 M
In the balanced reaction given below, how many grams of C14H9Cl5 (354.46 g/mol) will be produced by the reaction of 25.0 g of each of the starting materials? (C2HOCl3 = 147.38 g/mol, C6H5Cl = 112.6 g/mol)
C2HOCl3 + 2 C6H5Cl -> C14H9Cl5 + H2O
A) 354 g
B) 60.1 g
C) 121 g
D) 78.7 g
E) 39.4 g
E) 39.4 g
DAILY DOUBLE
Which of the following mixtures will result in a visible precipitate?
A) Ba(NO3)2(aq)+NaOH(aq)
B) Mg(NO3)2(aq)+NaOH(aq)
C) Sr(NO3)2(aq)+KOH(aq)
D) Ca(NO3)2(aq)+LiOH(aq)
B) Mg(NO3)2(aq)+NaOH(aq)
Which combination is correct for the reaction represented by this equation?
Cu(s) + Zn2+ (aq) -> Zn(s) + Cu2+ (aq)
A) Oxidized: Cu, Reduced: Zn2+
B) Oxidized: Cu2+, Reduced: Zn
C) Oxidized: Zn, Reduced: Cu+2
D) Oxidized: Zn+2, Reduced: Cu
E) Oxidized: Cu, Reduced: Cu+2
A) Oxidized: Cu, Reduced: Zn2+
Select the reaction that shows lead-210 decaying by emission of an alpha particle.
A) 82210Pb -> 80206Hg + 24He
B) 82210Pb -> 84214Po + 24He
C) 82210Pb + 0-1e -> 81210Ti
D) 82210Pb -> 83210 Bi + 0-1e
E) 82210Pb + 24He -> 84214Po
A) 82210Pb -> 80206Hg + 24He
DAILY DOUBLE
A sample of a simple hydrocarbon (a molecule composed of only carbon and hydrogens) was subjected to combustion analysis, producing 0.8594 g CO2 (44.01 g/mol) and 0.4399 g H2O (18.016 g/mol). What is the empirical formula of the hydrocarbon?
A) CH3
B) C4H5
C) C2H5
D) C3H2
E) C2H2
C) C2H5
100.g sulfuric acid (H2SO4, g/mol = 98.09) reacts with 65.00g lithium hydroxide (LiOH, g/mol = 23.95) to produce lithium sulfate (Li2SO4, g/mol=109.95) and water according to the balanced equation below.
H2SO4 (aq) + 2 LiOH (aq) -> Li2SO4 (aq) + 2 H2O
How many grams of H2SO4 will remain after the reaction has finished?
How many grams of LiOH will remain after the reaction has finished?
0g H2SO4. 16.19~g LiOH
What is the formula of the precipitate that forms when aqueous Potassium Phosphate (K3PO4) and aqueous Sodium Nitrate (NaNO3) are mixed?
A) Na3PO4
B) KNO3
C) NaK(PO4)2
D) K3(NO3)3
E) No precipitate forms.
E) No precipitate forms.
What species is the oxidation agent in the following reaction?
2 Cr2+(aq) + Co2+(aq) -> 2 Cr3+(aq) + Co(s)
A) Cr2+
B) Co2+
C) Cr3+
D) Co
E) There is no oxidation/reduction taking place.
B) Co2+
DAILY DOUBLE
A radioisotope of Fluorine-18 (18F) lies below the band of stability and thus neutron poor. It will most likely decay by
A) Alpha emission
B) Beta emission
C) spontaneous/induced fission
D) position emission or electron capture
E) neutron emission
D) position emission or electron capture
What is the balanced combustion reaction for Ethane (C2H6)?
2C2H6 +7O2 → 4CO2 +6H2O
What is the concentration of an HCl solution
if 25.00 mL HCl is titrated with 2.000 M NaOH? The initial burette reading is 2.13 mL, and the final burette reading after the titration finished is 39.42 mL.
A. 0.298 M
B. 1.49 M
C. 0.745 M
D. 3.15 M
E. 2.98 M
E. 2.98 M
A student has a clear, colorless aqueous solution of Lead (II) Nitrate (Pb(NO2)2). They perform two separate experiments:
Experiment 1: They add a few drops of 0.1 M HCl. A white precipitate forms.
Experiment 2: They take the same white precipitate from Experiment 1, add it to a beaker of pure distilled water, and heat the water to boiling. The precipitate completely disappears.
Which statement best explains these observations?
A) The precipitate is Pb(NO3)2, which is only soluble in acidic conditions.
B) The precipitate is PbCl2, which is an exception to the chloride rule and has a temperature-dependent solubility.
C) The precipitate is PbCl4, which is insoluble at all temperatures.
D) No precipitate actually formed; the cloudiness was just due to the density of the HCl.
B) The precipitate is PbCl2, which is an exception to the chloride rule and has a temperature-dependent solubility.
Write the total ionic and net ionic equation for this reaction. Include correct stoichiometric coefficients, charges, and states of matter.
Pb(NO3)2 (aq) + 2 KBr (aq) -> PbBr2 (s) + 2 KNO3 (aq)
Total ionic
Pb 2+aq + 2 NO3-aq + 2K+aq + 2Br-aq -> PbBr2s + 2K+aq + 2NO3-aq
Net ionic
Pb2+aq + 2Br-aq -> PbBr2(s)
Which of the following is a strong acid?
A) HF
B) HNO2
C) (HSO4)-
D) HClO4
E) H2S
D) HClO4