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Chem Final
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Questions in this quiz (35)
1Which of the following is an illustration of law of constant composition?
- AWater boils at 100 degrees C at 1 atm pressure.
- BWater is 11% hydrogen and 89% oxygen by mass.
- CWater can be separated into other substances by chemical process.
- DWater and salt have different boiling points.
- EWater is a compound.
2Of the following, ___________ is the largest mass.
- A25kg
- B2.5 x 10^-2 mg
- C2.5 x 10^15 pg
- D2.5 x 10^9 fg
- E2.5 x 10^10 ng
3How many atoms of nitrogen are in 10. g of NH4NO3?
- A3.5
- B1.5 X 10^23
- C3.0 X 10^23
- D1.8
- E2.0
4Propane (C3H8) reacts with oxygen in the air to produce carbon dioxide and water. In a particular experiment, 38.0 grams of carbon dioxide are produced from the reaction of 22.05 grams of propane with excess oxygen. What is the %yield in this reaction?
C3H8 + O2(g) -----> Ca(OH)2(aq) + H2(g)- A38.0
- B57.6
- C66.0
- D86.4
- E94.5
5Which of following equation is balanced, the coefficient of H2O is ______.
Ca(s) + H2O(I)----> Ca(OH)2(aq)+h2(g)- A1
- B2
- C3
- D5
- E4
6The element X has three naturally occurring isotopes. The masses ( amu) and % abundances of the isotopes are given in the table below. The average atomic mass of the element is ______ amu.
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Isotopes %Abundance Mass(amu)
221X 74.22 220.9
220X 12.78 . 220.0
218X 13.00 218.1- A219.7
- B220.5
- C220.42
- D218.5
- E221.0
7Aluminum reacts with a certain nonmetallic element to form a compound with the general formula Al2X3. Element X must be from Group ________ of the Periodic table of elements.
- A3A
- B4A
- C5A
- D6A
- E7A
8Which of the following are combustion reactions?
1) Ch4(g) + O2(g) ---> CO2(g) + H2O(I)
2) CaO(s) + Co2(g) ---> CaCo3(s)
3) PbCO3(s) ---> PbO(s) + CO2(g)
4) Ch3OH(I) + O2(g) ---> CO2(g) + H2O(I)- A1 and 4
- B1, 2, 3, and 4
- C1, 3, and 4
- D2, 3, and 4
- E3 and 4
9Calculate the percentage by mass of ammonia in cisplatin, PtCl2(NH3)2.
- A5.68
- B11.35
- C4.67
- D12.53
- E18.09
10The electron-domain geometry of ________ is tetrahedral.
- ACBr4
- BPH3
- CCCl2Br2
- DXeF4
- Eall of the above except XeF4
11Determine the reducing agent in the following reaction.
2Li(s) + Fe(C2H3O2)2(aq) ---> 2LiC2H3O2(aq) + Fe(s)- AO
- BH
- CC
- DFe
- ELi
12The net ionic equation for the reaction between aqueous sulfuric acid and aqueous sodium hydroxide is ______.
- AH+(aq) + HSO4- (aq)+2OH-(aq) ---> 2H2O(I) + SO4^2-(aq)
- BH+ (aq) + HSO4- (aq) + 2NA+ (aq) + 2OH- (aq) ---> 2H2O(I) + 2Na+ (aq) + So4^2(aq)
- CSO4^2- (aq) + 2Na+(aq) +SO42- (aq)
- DH+(aq) + OH-(aq) ----> H2O(I)
- E2H+ (aq) + SO4^2- (aq) + 2Na + (aq) +2OH- (aq) ---> 2H2O (I) + 2Na+ (aq) +SO4^2- (aq)
13One method for removal of metal ions from a solution is to convert the metal to its elemental form so it can be filtered out as a solid. Which metal can be used to remove aluminum ions from solution?
- Azinc
- Bcobalt
- Clead
- Dcopper
- Enone of these.
14Which of the following is a statement of the first law of thermodynamics.
- AEk= 0.5mv^2
- Ba negative △H correspond to an exothermic process.
- C△E= E final - Eintial
- DEnergy lost by the system must be gained by the surroundings.
- E1 cal = 4.184 J (exactly)
15Which of the following is a statement of Hess's law?
- AIf a reaction is carried out in a series of steps, the △H for the reaction will equal the sum of the enthalpy changes for the individual steps.
- BIf a reaction is carried out in a series of steps, the △H for the reaction will equal the product of the enthalpy changes for the individual steps.
- CThe △H for a process in the forward direction is equal in magnitude and opposite in sign to the △H for the process in the reverse direction.
- DThe △H for a process in the forward directions is equal to the △H for the process in the reverse direction.
- EThe △H of a reaction depends on the physical states of the reactants and products.
16Deter the specific heat capacity of an alloy that requires 69.3 kJ to raise the temperature of 150.0g alloy from 450K to 550K.
- A3.20 J/g °C
- B2.00 J/g°C
- C4.62 J/g°C
- D1.79 J/g°C
- E7.20 J/g°C
17Given the data in the table below, △H° rxn for the following reactions is _______kJ.
Ca(OH)2(s) + 2HCl(aq) ----> CaCl2(aq) + 2H2O(I)
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Substances ] △Hf°(kJ. mol^-1)
Ca(OH)2(s) ] -986.09
HCl(aq) ] -167.159
CaCl2(aq) ] -877.13
H2O(I) ] -285.83- A-744.9
- B-4519
- C-164.59
- D-130.42
- E-128.38
18The formal charge on carbon in the molecule below is _______.
.. ..
O = C = O
.. ..- A0
- B+1
- C+2
- D+3
- E-1
19The hybridizations of iodine in IF3 is ________.
- Asp
- Bsp²
- Csp³
- Dsp³d
- Esp³d²
20The π bond in ethlene, H2C=CH2, results from the overlap of _______.
- Asp3 hybrid orbitals
- Bs atomic orbitals
- Csp hybrid orbitals
- Dsp^2 hybrid orbitals
- Ep atomic orbitals
21With what compound will NH3 experience only ion-dipole intermolecular forces?
- ALiCl
- BSiH4
- CCH3I
- DC3H7OH
- EOCl2
22Which combination will produce a precipitate?
- ANH4OH (aq) and HCl(aq)
- BAgNO3(aq) and Ca(C2H3O2)2(aq)
- CNaOH (aq) and HCl(aq)
- DNaCl (aq) and HC2H3O2(aq)
- ENaOH(aq) and Fe(NO3)2 (aq)
23Based on the following information, which compound has the strongest intermolecular forces?
Substance ▵Hvap(kJ/mol)
Argon(Ar) 6.3
Benzene(C6H6) 31.0
Ethanol ( C2H5OH) 39.3
Water (H2O) 40.8
Methane (CH4) 9.3- AArgon
- BBenzene
- CEthanol
- DWater
- EMethane
24The molecular weight of a gas that has a density of 7.10 g/L at 25.0°C and 1.00 atm pressure is _______g/mol.
- A174
- B14.6
- C28.0
- D5.75 x 10^-³
- E6.85 x 10^-²
25Which of the following does not have eight valence electrons?
- ACa+
- BRb+
- CXe
- DBr-
- EAll of the above have eight valence electrons.
26In ionic bond formation, the lattice energy of ions _______ as the magnitude of the ion charges _________ and the radii _______.
- Aincreases, decreases, increase
- Bincreases, increase, increase
- Cdecreases, increase, increase
- Dincreases, increase, decrease
- Eincreases, decrease, decrease
27Which of the following is correctly matched?
- A(NH4)sCO3, diammonium carbonate;
- BAl2S3 aluminum (III) sulfide;
- CH2CO3 carbonic acid;
- DH2S(aq) hydrogen sulfide;
- EKOH(aq), sodium oxygen hydrogen.
28The lewis structure of PF3 shows that the central phosphorus atom has _______ nonbonding and ______ bonding electron pair(s).
- A2, 2
- B1, 3
- C3, 1
- D1, 2
- E3, 3
29What is the electron configuration for the Mn ^2+ ion?
- A[Ar] 4s¹3d⁶
- B[Ar]3d⁷
- C[Ar]3d⁵
- D[Ar]4s²3d⁹
- E[Ne]3s²3p¹⁰
30Which species has London dispersion forces as the only intermolecular force?
- AAr
- BHbr
- CCH3CH2OH
- DNH3
- EH2O
31Determine the molarity of a solution formed by dissolving 97.7 g LiBr in enough water to yield 750.0 mL of solution.
- A1.50 M
- B1.18 M
- C0.130 M
- D0.768 M
- E2.30 M
32Ammonium nitrite undergoes thermal decomposition to produce only gases.
NH4NO2(s) ----> N2(g) +2H2O(g)
What volume (L) of has is produced by the decomposition of 35.0g of NH4NO2(s) at 400°C and 1.5 atm?- A60.0
- B20.0
- C15.1
- D72.0
- E24.0
33According to kinetic-molecular theory, if the temperature of a has is raised from 100°C to 200°C, the average kinetic energy of the gas will _______.
- Adouble
- Bincrease by a factory of 1.27
- Cincrease by a factor of 100
- Ddecrease by half
- Edecrease by a factor of 100
34Of the following, which gives the correct order for atomic radius for Mg, Na,P, Si, and Ar?
- AMg > Na > P > Si > Ar
- BAr > Si > P > Na > Mg
- CSi > P > Ar > Na > Mg
- DNa > Mg > Si > P > Ar
- EAr > P > Si > Mg > Na
35Which combination of protons, neutrons, and electrons is correct for the isotope of copper 63/29Cu²+.
- A29p+, 34 n°, 27e-
- B29p+, 29n°, 63 e-
- C63p+, 29n°, 63 e-
- D34p+,29n°,34 e-
- E34p+, 34n°, 27e-
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- Quiz on Chem Final, created by Tommy Bui on 06/12/2019.
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- Tommy Bui
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