Chemistry 2202 – Test 1 Review Sheet
1.
A 2.50 g piece of solid carbon dioxide (dry ice) is placed in a plastic bag. It warms to form carbon
dioxide gas. The sealed bag is maintained at STP conditions. Calculate the volume of gas in the
sealed bag.
2.
Determine the empirical formula of an antimony-sulfur compound that is 60.29% antimony and
39.71% sulfur.
3.
An ester which has fruity scent is analyzed by mass spectroscopy. It is found to have a molar
mass of 116.18 g/mol. Its percent composition is 62.02% carbon, 27.54% oxygen and 10.43%
hydrogen. Determine the molecular formula of this ester.
4.
For each isotope, list the # of protons, # of neutrons, # of electrons, mass # and atomic number
a.
b.
c.
d.
e.
5.
Carbon-12
Carbon-14
Vanadium-51
Cobalt-56
Zinc-65
Determine the molar mass of:
a. Sucrose, C12H22O11
b. Methane, CH4
c. Platinum(II)Phosphate
d. Calcium Nitride
e. Manganese Chlorate
6. Find the average atomic mass of a sample of Calcium which is 25.0% Ca-40 (39.99 amu) 45% Ca41 (40.95 amu) and 30.0% Ca-42 (41.94 amu)
7. What is the percent composition of a sample of Magnesium if it has an average atomic mass of
24.21 amu and is composed of Mg-24 (23.99 amu) and Mg-27 (26.90 amu)
8.
Find the:
a. Moles of radium metal in 3.45 x 1024 atoms.
b. Molecules of water in 10.5 moles.
c. Hydrogen atoms in 10.5 moles of water.
d. Volume of 3.4 mol of Nitrogen gas at STP
e. Volume of 3.4 mol of Nitrogen gas at SATP
f. Molecules of Nitrogen in 0.255L of gas at STP
g. Atoms of Nitrogen in 0.255L of nitrogen gas at STP
h. Mass of 2.456 mol of Barium Bromide
i. Moles of Mercury(II) Sulfate dehydrate in 600.5 g
j. Mass of 3.99 L of Chloroform Gas (CHCl3) at SATP.
9.
Calculate the percent composition of water of
a. Potassium Thiosulfate Dihydrate
b. Copper Chloride Tetrahydrate
10. For each reaction, find the number of moles of each product:
a. 2.00 mol of Fe
H2SO4 + Fe ---> Fe2(SO4)3 + H2
b.
3.4 mol of O2
Al + O2 ---> Al2O3
c. 1.45 x 106 mol of Mg3N2
Mg3N2 + H2O ---> MgO + NH3
11. For the reactions above, determine :
a. The volume of H2 gas produce when 55.4g of Fe is used (at STP)
b. The number of formula units of Al2O3 produced when 33.4 L of O2 gas is reacted at STP
c. The mass of water required to produce 100.0g of Ammonia.