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CHEM121 001 Final Test

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1.
Choose the one set of quantum numbers that does not contain an error. A) 
n = 4, l = 0, ml =-1 B) 
n = 3, l = 1, ml = -2 C) 
n = 5, l = 3, ml =-3 D) 
n = 4, l = 4, ml =0 E) 
n = 3, l = 2, ml =+3
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2.
The mass number is equal to?
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3.
What is the empirical formula for C4H10O2?
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4.
A mixture of N2, O2 and Ar have mole fractions of 0.25, 0.65, and 0.10, respectively. What is the pressure of N2 if the total pressure of the mixture is 3.9 atm?
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5.
Determine the velocity of a marble (m = 8.66 g) with a wavelength of 3.46 × 10-33 m.
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6.
Calculate the change in internal energy (ΔE) for a system that is absorbing 35.8 kJ of heat and is expanding from 8.00 to 24.0 L in volume at 1.00 atm. (Remember that 101.3 J = 1 L∙atm)
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7.
Choose the pure substance from the list below. 
air, 

sea water, 
milk, sugar, 
lemonade
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8.
Calculate the temperature, in K, of 2.20 moles of gas occupying 3.50 L at 3.30 atm.
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9.
Calculate the mass (in g) of 1.9 x 1024 atoms of Pb. 

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10.
Give the formula for sulfurous acid.
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11.
Write a balanced equation to show the reaction of aqueous aluminum acetate with aqueous ammonium phosphate to form solid aluminum phosphate and aqueous ammonium acetate.
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12.
Which of the following are examples of a chemical change? 
copper building materials develop a green patina over time 
a match burns 
ethanol evaporates 
Both A and B are examples of chemical change. All of the above
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13.
According to the following reaction, how much energy is required to decompose 55.0 kg of Fe3O4? The molar mass of Fe3O4 is 231.55 g/mol. Fe3O4(s) → 3 Fe(s) + 2 O2(g) ΔH°rxn = +1118 kJ
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14.

Determine the mass of an object that has a volume of 88.6 mL and a density of 9.77 g/mL.
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15.
Identify the correct values for a 3p sublevel.
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16.
Rank the following in order of decreasing rate of effusion. F2, SF6, CO, Kr
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17.
The statement, "In a chemical reaction, matter is neither created nor destroyed" is called?
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18.
Predict the charge that an ion formed from sulfur would have.
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19.
Identify HCl.
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20.
Use the standard reaction enthalpies given below to determine ΔH°rxn for the following reaction: 2 S(s) + 3 O2(g) → 2 SO3(g) ΔH°rxn = ? Given: SO2(g) → S(s) + O2(g) ΔH°rxn = +296.8 kJ 2 SO2(g) + O2(g) → 2 SO3(g) ΔH°rxn = -197.8 kJ
A.
2.66 × 105 kJ
B.

the sum of the number of protons and neutrons.
C.
H2SO3
D.

-791.4 kJ
E.
64.0 K
F.
866 grams
G.
the Law of Conservation of Mass.
H.
sugar
I.
C2H5O
J.
22.1 m/s
K.
CO > F2 > Kr > SF6
L.
strong electrolyte, strong acid
M.
Al(C2H3O2)3 (aq) + (NH4)3PO4 (aq) → AlPO4 (s) + 3 NH4C2H3O2 (aq)
N.
6.5 × 102 grams
O.
Both A and B are examples of chemical change.
P.
2-
Q.
+34.2 kJ
R.
0.98 atm
S.
n = 3, l = 1, ml = 0
T.
C
Type the Answer that corresponds to the displayed Question.
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21.

If a solution has a temperature of 355 K, what is its temperature in degrees celsius?
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22.
Give the structure for sodium chlorate.
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23.
Silver has an atomic mass of 107.868 amu. The Ag-109 isotope (108.905 amu) is 48.16%. What is the amu of the other isotope?
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24.
A gas is at 35.0°C and 4.50 L. What is the temperature at 9.00 L?
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25.
Which of the following contains BOTH ionic and covalent bonds?
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26.
Calculate the change internal energy (ΔE) for a system that is giving off 45.0 kJ of heat and is performing 855 J of work on the surroundings.
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27.
A sample of gas initially has a volume of 859 mL at 565 K and 2.20 atm. What pressure will the sample have if the volume changes to 268 mL while the temperature is increased to 815 K?
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28.
Determine the specific heat capacity of an alloy that requires 59.3 kJ to raise the temperature of 150.0 g alloy from 298 K to 398 K.
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29.
Write the name for Ca3(PO4)2.
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30.
A syringe contains 0.65 moles of He gas that occupy 750.0 mL. What volume (in L) of gas will the syringe hold if 0.35 moles of Ne is added?

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