Test 2 Review
Name:
Question 1. (3 pts) If 93.5L of a gas at -43.8◦C has a pressure of 0.835atm, what is the final temperature
in ◦C if the pressure is increased to 850mmHg and the volume decreased to 40.0L?
Question 2. (4 pts) What is the pressure (in mmHg) of a gas that occupies 872.3mL, has a temperature
of 67.3◦C and contains 1.76 moles of N2?
Question 3. (4 pts) At standard temperature and pressure (STP), how many moles of N2 occupy
1.43x109μL?
Question 4. (4 pts) What volume (in L) is occupied by 2.34 moles of Xe gas at 12 ◦C at a pressure of
657mmHg?
Question 5. Draw the electron dot formulas for the following:
a) CCl2H2 (Carbon is central atom)
b) PF3
c) For the compounds in question #5, give the number of electron groups, the electronic geometry
and the molecular shape of the molecules.
Compound
Electron
Groups
Electron
Molecular
Group
Shape
Arrangement
CCl2H2
PF3
Question 6. Write the molecular formula for the following names:
a) Iron (IV) Oxide
b) Vanadium (V) Phosphate
c) Barium Phosphide
d) Calcium sulfide
e) Disulfur trioxide
f) Phosphorus dinitride
Question 7. Name the following covalent compounds:
a) SiCl4
b) Trifluorine pentasulfide
Question 8. If 55.2g of N2 and 75.3g of O2 are reacted to form laughing gas, N2O:
a) What is the balanced chemical equation for the formation of laughing gas?
b) What is the limiting reactant?
c) How much laughing gas is produced(in grams)?
d) What is the percent yield if only 72.5g of N2O are collected?
Question 9. Consider the reaction:
2Fe(s) + AuCl4(aq) → Au(s) + 2FeCl2(aq)
a) What type of reaction is it?
b) What species is being reduced and what is being oxidized?
Question 10. Consider the Molecule NaH2PO4:
a) What is its Molar Mass?
b) How many moles are in 234.5g of it?
c) How many moles are 8.36x1022 molecules?
d) How many H atoms are in 2.73x10-9 moles?
e) How many O atoms are in 7.35 moles?
Question 11. Write the Balanced Formulas for the following Anions and Cations:
O2Ba2+
Fe4+
V5+
Na+
OHFe3+
N3-
ClO-
Gas Law Equations:
P1V1=P2V2
V1=V2
T1 T2
P1 = P2
T1 T2
V1 = V2
n1 n2
P1V1=P2V2
T1 T2
PV=nRT where R=0.0821(L●atm)/(mole●K) or,
R=62.4 (L●mmHg)/(mole●K)