Chem 1010 - General Chemistry 1 » Summer 2021 » Final Exam (B)
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Question #1
What pressure would a gas mixture in a 10.0 L tank exert if it were composed of 48.5 g He and 94.6 g CO 2 at 398 K?
A.
58.7 atm
B.
32.6 atm
C.
7.02 atm
D.
46.6 atm
E.
39.6 atm
Question #2
A 0.286-g sample of gas occupies 125 mL at 60. cm of Hg and 25°C. What is the molar mass of the gas?
A.
5.9 g/mol
B.
59 g/mol
C.
44 g/mol
D.
71 g/mol
Question #3
Which of the following statements is TRUE?
A.
A strong acid is composed of a proton and an anion that have a very strong attraction for one another.
B.
The conjugate base of a very weak acid is stronger than the conjugate base of a strong acid.
C.
A weak base is composed of a cation and an anion with a very weak attraction between them.
D.
A strong acid has a strong conjugate base.
E.
None of the above statements are true.
Question #4
Which of the following is a Br ℯnsted-Lowry acid?
A.
NH2-
B.
CH4
C.
NH3
D.
Br2
E.
NH4+
Question #5
Which of the following statements is TRUE?
A.
Part of the Bohr model proposed that electrons in the hydrogen atom are located in "stationary states" or particular orbits around the nucleus.
B.
An orbital is the volume in which we are most likely to find an electron. Part of the Bohr model proposed that electrons in the hydrogen atom are located in "stationary states" or particular orbits around the nucleus. The uncertainty principle states that we can never know both the exact location and speed of an electron. The emission spectrum of a particular element is always the same and can be used to identify the element.
C.
The uncertainty principle states that we can never know both the exact location and speed of an electron.
D.
The emission spectrum of a particular element is always the same and can be used to identify the element.
E.
An orbital is the volume in which we are most likely to find an electron.
Question #6
Calculate the wavelength (in nm) of a the red light emitted by a neon sign with a frequency of 4.92 × 10 14 Hz.
A.
192 nm
B.
792 nm
C.
492 nm
D.
164 nm
E.
610 nm
Question #7
Which statement is FALSE?
A.
ΔErxn is a measure of heat.
B.
ΔHrxn is the heat of reaction.
C.
An exothermic reaction gives heat off heat to the surroundings.
D.
Endothermic has a positive ΔH.
E.
Enthalpy is the sum of a system's internal energy and the product of pressure and volume.
Question #8
A piece of iron (C=0.449 J/g°C) and a piece of gold (C=0.128 J/g°C) have identical masses. If the iron has an initial temperature of 498 K and the gold has an initial temperature of 298 K, which of the following statements is TRUE of the outcome when the two metals are placed in contact with one another? Assume no heat is lost to the surroundings.
A.
Since the two metals have the same mass, the final temperature of the two metals will be 398 K, exactly halfway between the two initial temperatures.
B.
Since the two metals have the same mass, the thermal energy contained in each metal after equilibrium will be the same.
C.
Since the two metals have the same mass, but the specific heat capacity of gold is much smaller than that of iron, the final temperature of the two metals will be closer to 298 K than to 498 K.
D.
Since the two metals have the same mass, the thermal energy contained in the iron and gold after reaching thermal equilibrium will be the same.
E.
None of the above are true.
Question #9
A 100.0 mL sample of 0.300 M NaOH is mixed with a 100.0 mL sample of 0.300 M HNO 3 in a coffee cup calorimeter. If both solutions were initially at 35.00°C and the temperature of the resulting solution was recorded as 37.00°C, determine the ΔH° rxn (in units of kJ/mol NaOH) for the neutralization reaction between aqueous NaOH and HCl. Assume 1) that no heat is lost to the calorimeter or the surroundings, and 2) that the density and the heat capacity of the resulting solution are the same as water.
A.
-16.7 kJ/mol NaOH
B.
- 34.4 kJ/mol NaOH
C.
-55.7 kJ/mol NaOH
D.
-27.9 kJ/mol NaOH
E.
-169 kJ/mol NaOH
Question #10
What mass (in mg) does 2.63 moles of nickel have?
A.
2.23 × 104 mg
B.
3.56 x 105 mg
C.
44.8 mg
D.
1.54 x 105 mg
E.
129 mg
Question #11
Which of the following statements about subatomic particles is TRUE?
A.
Neutrons and electrons are found in the nucleus of an atom.
B.
A neutral atom contains the same number of protons and electrons.
C.
Protons have about the same mass as electrons.
D.
Protons and neutrons have opposite, but equal in magnitude, charges.
E.
Electrons make up most of the mass of an atom.
Question #12
An alligator is 152.4 cm long. How long is he in feet?
A.
32.2 ft
B.
12.7 ft
C.
720.0 ft
D.
60.0 ft
E.
5.00 feet
Question #13
Gas is sold for $1.399 per liter in Toronto, Canada. Your car needs 12.00 gallons. How much will your credit card be charged in Canadian dollars?
A.
$16.79
B.
$63.54
C.
$4.44
D.
$67.15
Question #14
In an acid-base neutralization reaction 38.74 mL of 0.500 M potassium hydroxide reacts with 50.00 mL of sulfuric acid solution. What is the concentration of the H 2SO 4 solution?
A.
0.387 M
B.
1.29 M
C.
0.194 M
D.
0.775 M
Question #15
How many grams of CaCl 2 are formed when 15.00 mL of 0.00237 M Ca(OH) 2 reacts with excess Cl 2 gas? 2 Ca(OH) 2( aq) + 2 Cl 2( g) → Ca(OCl) 2( aq) + CaCl 2( s) + 2 H 2O( l)
A.
0.00394 g
B.
0.0507 g
C.
0.00197 g
D.
0.00789 g
Question #16
How many grams of H 2 gas can be produced by the reaction of 54.0 grams of Al( s) with an excess of dilute hydrochloric acid in the reaction shown below? 2 Al( s) + 6 HCl( aq) → 2 AlCl 3( aq) + 3 H 2( g)
A.
12.1 g
B.
2.68 g
C.
6.05 g
D.
4.04 g
Question #17
Determine ΔH vap for a compound that has a measured vapor pressure of 24.3 torr at 273 K and 135 torr at 325 K.
A.
34 kJ/mol
B.
13 kJ/mol
C.
79 kJ/mol
D.
24 kJ/mol
E.
41 kJ/mol
Question #18
Determine the vapor pressure (in torr) of a substance at 36°C, whose normal boiling point is 84°C and has a ΔH vap of 22.1 kJ/mol.
A.
41.8 torr
B.
147 torr
C.
239 torr
D.
31.8 torr
E.
98 torr
Question #19
What is the molecular geometry of NCl 3?
A.
trigonal planar
B.
trigonal pyramidal
C.
T-shaped
D.
tetrahedral
Question #20
How many of the following molecules are polar? BrCl 3 CS 2 SiF 4 SO 3
A.
0
B.
1
C.
2
D.
4
E.
3
Question #21
Give the reason that antifreeze is added to a car radiator.
A.
The freezing point is elevated and the boiling point is lowered.
B.
The freezing point is lowered and the boiling point is elevated.
C.
The freezing point and the boiling point are elevated.
D.
The freezing point and the boiling point are lowered.
E.
None of the above.
Question #22
Calculate the freezing point of a solution of 40.0 g methyl salicylate, C 7H 6O 2, dissolved in 800. g of benzene, C 6H 6. Kf for the benzene is 5.10 ⁰C/m and the freezing point is 5.50°C for benzene.
A.
3.41°C
B.
-2.09°C
C.
7.59°C
D.
2.09°C
Question #23
To make a 0.500 M solution, one could take 0.500 moles of solute and add
A.
enough solvent to make 1.00 kg of solution.
B.
1.00 L of solvent.
C.
enough solvent to make 1.00 L of solution.
D.
1.00 kg of solvent.
Question #24
Choose the bond below that is most polar.
A.
H-Br
B.
H-Cl
C.
H-F
D.
C-H
E.
H-I
Question #25
How many lone pairs of electrons are on the S atom in SF 4 ?
A.
3
B.
2
C.
1
D.
0
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