Download ADVANCED CHEMISTRY WKST

AP CHEMISTRY WKST
SEMESTER 1 REV.—PROBLEMS
NAME: ______________________________________
1. Determine the mass percent of the elements in CuSO 4·5H2O.
2. Determine the empirical formula for the compound composed of 43.7% P and 56.3% O.
3. A 1.025 g sample of a compound containing only carbon and hydrogen was burned to give 3.007 g CO 2 and 1.845 g
H2O. What is the empirical formula of the compound?
4. A substance has an empirical formula of CH2 and a molar mass of 56.0 g/mol. What is the molecular formula of the
compound?
5. For the reaction: 5HClO3 + HCl  6ClO2 + 3H2O
a) Determine the mass of HClO3 needed to make 50.00 g ClO2.
b) If 53.245 mL of a 1.25 M HCl solution reacted, what mass of H2O formed?
c) Determine the mass of H2O formed if 50.00 g of HClO3 is mixed with 25.00 g HCl. What is the limiting reactant?
d) Determine the theoretical yield of ClO2 if 100.0 mL of a 0.75 M HClO3 solution is mixed with 50.0 mL of 1.125 M
HCl solution.
e) If the given reaction has ΔH = 135 kJ/mol, what is the amount of heat released if 25.0 g HClO 3 reacted?
6. What is the mass of Fe in 25.0 g of Fe2O3?
7. Write the ionic and net ionic equations for:
a) 2Al(NO3)3(aq) + 3K2CO3(aq)  6KNO3(aq) + Al2(CO3)3(s)
b) H2CO3(aq) + Ba(OH)2(aq)  BaCO3(s) + 2H2O(l)
8. Balance the following equations.
a) Fe2O3 + LiBr  FeBr3 + Li2O
b) C6H14 + O2 → CO2 + H2O
c) Na3PO4 + Zn(NO3)2 → Zn3(PO4)2 + NaNO3
d) C3H7OH + Na2Cr2O7 + H2SO4  Cr2(SO4)3 + Na2SO4 + H2O + HC3H5O2
9. Complete the following equations—include the physical states but you do not have to balance them.
a) sodium carbonate solution is mixed with a silver nitrate solution
b) solid potassium metal is mixed with an iron(III) nitrate solution
c) sulfuric acid reacts with solid calcium carbonate
d) solid potassium sulfide reacts with nitric acid
e) solid sodium oxide is placed in water
f) solid strontium oxide reacts with sulfur trioxide gas
g) solid ammonium nitrate reacts with potassium hydroxide solution
10. Balance the redox equation for a basic solution: As 2O3 + NO3ˉ  H3AsO4 + N2O3
11. A 4.500 L sample of an ideal gas at 10.0C and 2.25 atm was compressed to 0.1244 L against an external pressure
of 10.0 atm. If the temperature remained 10.0C and ΔH for this process was 1020 J, determine ΔE for the system.
12. A 50.00 g sample of a metal was heated to 99.5C and then placed into a calorimeter containing 75.0 mL of H2O at
23.0C. If the final temperature of the mixture reached 38.2C, determine the specific heat of the metal.
13. Determine the standard enthalpy of formation for the reaction: 4NO2(g) + 6H2O(l)  4NH3(g) + 7O2(g)
(Look in appendix for values.)
15
14. Determine the frequency of an electromagnetic wave with a wavelength of 3.2 x 10ˉ
th
rd
m.
15. Determine ΔE for an electron going from the 10 energy level to the 3 energy level and then determine the
wavelength for the resulting photon.
-216. Determine ΔH for the reaction 2B(s) + 3H 2(g)  B2H6(g) given the following mechanism.
3
2
O2(g)  B2O3(s)
ΔH = 1273 kJ
B2H6(g) + 3O2(g)  B2O3(s) + 3H2O(g)
ΔH = 2035 kJ
2B(s) +
H2(g) +
1
2
O2(g)  H2O(l)
ΔH = 286 kJ
H2O(l)  H2O(g)
ΔH = +44 kJ
17. Determine the wavelength of a particle having a mass of 2.225 x 10ˉ
31
kg moving at 20.0% of the speed of light.
18. A gas is collected over water at 20.00°C and 745.25 torr. If the original sample was 11.23 L, what would the volume
be at STP for the “dry” gas?
19. What would the pressure be, in kPa, if a 33.5 g sample of N2 occupied 20.25 L at −12.25°C?
–
20. Draw the Lewis structure, draw the molecular shape, and determine the polarity of CCl4, NO2 , ICl4 , BrF5
+
21. Write the complete dissociation equations for the following.
a) Na2SO4
b) HNO3
c) H2CrO4
22. In the reaction 4Fe(OH)2 + O2 + 2H2O → 4Fe(OH)3, determine the element undergoing oxidation and reduction and
determine the oxidizing and reducing agents.
23. Determine the density of SO3 at 25.0°C and 810.0 torr.
24. A can is filled with 15.55 g CO2 and 17.88 g O2. If the pressure inside the can is 1.354 atm, what is the partial
pressure of the CO2?
25. A 4.000 g sample of a gas occupies 6.50 L at STP. Determine its molar mass.
26. Calculate the energy of interaction, in kJ/mol, for the bonds in MgCl2 if the internuclear distance is 39.5 nm.
27. Write the set of quantum numbers for the first 4 electrons filling the 4p sublevel.
28. Draw the orbital diagram for Ru (core method acceptable).
5+
3–
29. Write the electron configuration for: Cr, As , P , Pb (core method acceptable)
30. Name the following compounds.
a) V2O5
b) (NH4)2C2O4
c) Po(SCN)6
d) P4O10
e) Zn(OH)2
f) KCN
g) Cs2C4H4O6
h) Li3BO3
i) Hg(C2H3O2)2
j) [Ag(NH3)2]Cl
k) (NH4)3[Fe(SCN)6]
l)
m)
n)
o)
p)
q)
r)
s)
t)
u)
v)
Ag2CrO4
SnCO3
NaHCO3
Mn2O7
Cu(H2PO4)2
Fr2Cr2O7
[Co(NH3)3(H2O)3]Cl3
Hg2(NO3)2
Ce(C6H5COO)4
KHC8H4O4
K2[Cu(CN)4]
-331. Write the formula for the following compounds.
a) iron(II) sulfite
b) cupric nitrate
c) mercury(I) chloride
d) tetraamminezinc nitrate
e) potassium chlorate
f) magnesium carbonate
g) barium peroxide
h) potassium sulfate
i) tin(IV) oxide
j) plumbous hydroxide
k) nickel(II) phosphate
l) silver diaquotetrakis(sulfato)stannate(IV)
32. Name the following acids.
a) HBr
b) H2SO4
c) H3PO4
d) H2C2O4
e) HCl
f) H2Cr2O7
g) H2CO3
33. Write the formula for the following acids.
a) sulfurous acid
b) hydrofluoric acid
c) hydriodic acid
d) boric acid
e) hydrocyanic acid
f) perchloric acid
g) iodic acid
m)
n)
o)
p)
q)
r)
s)
t)
u)
v)
w)
x)
copper(I) acetate
dinitrogen tetroxide
hexaamminecopper(II) pentacyanohydroxoferrate(III)
rubidium phosphide
sulfur hexafluoride
iron(III) oxide
ammonium sulfite
calcium permanganate
phosphorus pentafluoride
lithium hydride
titanium(IV) hydrogen phosphate
potassium hexacyanocobaltate(III)