Chapter 3 Practice Test Flashcards
Which one of the following chemical equations is balanced?
SO3 + H2O → H2SO4
Which of the following represents a balanced chemical equation for the word equation below?
iron(II) sulfide + hydrochloric acid → iron(II) chloride + hydrogen sulfide
FeS + 2HCl → FeCl2 + H2S
In the following balanced chemical equation,
2Al(OH)3 + 3H2 SO4 → Al2(SO4 )3 + 6H2 O
what is the ratio of water molecules produced per molecule of sulfuric acid in the reaction?
2 molecules of water per molecule of sulfuric acid
Calcium carbonate reacts with hydrochloric acid to produce calcium chloride, water, and carbon dioxide. Which of the following balanced chemical equations represents this reaction?
CaCO3 + 2HCl → CaCl2 + H2O + CO2
Balance the following chemical reaction:
NaHCO3 → Na2CO3 + H2O + CO2
2NaHCO3 → Na2CO3 + H2O + CO2
Balance the following chemical reaction for the decomposition of nitroglycerin to form many moles of different gases.
C3H5N3O9 → N2 + CO2 + H2O + O2
4C3H5N3O9 → 6N2 + 12CO2 + 10H2O + O2
How many molecules of carbon dioxide are found in 2.50 moles of carbon dioxide?
1.51 × 10^24 molecules
How many atoms of hydrogen, sulfur, and oxygen are in 1.00 mol of H2SO4?
- 20 × 10^24 hydrogen;
- 02 × 10^23 sulfur;
- 41 × 10^24 oxygen
How many atoms of uranium are there in 7.11 millimoles of this substance?
4.28 × 10^21 atoms
What mass does 0.876 moles of hydrogen peroxide (H2O2 ) represent?
29.8 grams
In the portion of the periodic table shown, what does the number 12.0107 represent?
molar mass
What is the molar mass of ethanol (C2H6O)?
46.064 grams / mole
When the mass percent of each element making up an unknown compound is given, what other information is needed to determine the empirical formula?
the molar mass of each element
The mineral zircon contains the following elements in the mass proportions indicated:
49. 8% Zr 15. 3% Si 34. 9% O
What is the empirical formula of zircon?
ZrSiO4
What is the minimum information necessary in order to determine the molecular formula of an unknown compound?
the empirical formula plus the molecular weight of the compound