Chem Exam 2

The balanced molecular equation for complete neutralization of H2SO4 by KOH in aqueous solution is __________.
A) 2H+ (aq) + 2OH- (aq) → 2 H2O (l)
B) 2H+ (aq) + 2KOH (aq) → 2 H2O (l) + 2K+ (aq)
C) H2SO4 (aq) + 2OH- (aq) → 2 H2O (l) + SO42- (aq)
D) H2SO4 (aq) + 2KOH (aq) → 2 H2O (l) + K2SO4 (s)
E) H2SO4 (aq) + 2KOH (aq) → 2 H2O (l) + K2SO4 (aq)

Click the card to flip 👆

1 / 58

Terms in this set (58)

E) H2SO4 (aq) + 2KOH (aq) → 2 H2O (l) + K2SO4 (aq)

The net ionic equation for formation of an aqueous solution of Al(NO3)3 via mixing solid Al(OH)3 and aqueous nitric acid is __________.
A) Al(OH)3 (s) + 3HNO3 (aq) → 3 H2O (l) + Al(NO3)3 (aq)
B) Al(OH)3 (s) + 3NO3- (aq) → 3OH- (aq) + Al(NO3)3 (aq)
C) Al(OH)3 (s) + 3NO3- (aq) → 3OH- (aq) + Al(NO3)3 (s)
D) Al(OH)3 (s) + 3H+ (aq) → 3 H2O (l) + Al3+ (aq)
E) Al(OH)3 (s) + 3HNO3 (aq) → 3 H2O (l) + Al3+ (aq) + NO3- (aq)

D) Al(OH)3 (s) + 3H+ (aq) → 3 H2O (l) + Al3+ (aq)

Which combination will produce a precipitate?
A) NH4OH (aq) and HCl (aq)
B) AgNO3 (aq) and Ca(C2H3O2)2 (aq)
C) NaOH (aq) and HCl (aq)
D) NaCl (aq) and H C2H3O2 (aq)
E) NaOH (aq) and Fe(NO3)2 (aq)

E) NaOH (aq) and Fe(NO3)2 (aq)

Which of these metals will be oxidized by the ions of cobalt?
A) nickel
B) tin
C) iron
D) copper
E) silver

C) iron

What volume (mL) of 0.135 M NaOH is required to neutralize 13.7 mL of 0.129 M HCl?
A) 13.1
B) 0.24
C) 14.3
D) 0.076
E) 6.55

A) 13.1

What are the spectator ions in the reaction between Mg(OH)2 (aq) and HCl (aq)?
A) Mg+2 and H+
B) H+ and OH-
C) Mg+2 and Cl-
D) H+ and Cl-
E) OH- only

C) Mg+2 and Cl-

When aqueous solutions of AgNO3 and NaCl are mixed, AgCl precipitates. The balanced net ionic equation is __________.
A) Ag+ (aq) + Cl- (aq) → AgCl (s)
B) Ag+ (aq) + NO3- (aq) → AgNO3 (s)
C) Ag+ (aq) + NO3- (aq) → AgNO (aq)
D) AgNO3 (aq) + NaCl (aq) → AgCl (s) + NaNO3 (aq)
E) AgNO3 (aq) + NaCl (aq) → AgCl (aq) + NaNO3 (s)

A) Ag+ (aq) + Cl- (aq) → AgCl (s)

Which of these metals is the most easily oxidized?

Na
Au
Fe
Ca
Ag
A) Na
B) Au
C) Fe
D) Ca
E) Ag

D) Ca

The molarity (M) of an aqueous solution containing 52.5 g of sucrose (C12H22O11) in 35.5 mL of solution is __________.
A) 5.46
B) 1.48
C) 0.104
D) 4.32
E) 1.85

D) 4.32

How many grams of CH3OH must be added to water to prepare 150 mL of a solution that is 1.0 M CH3OH?
A) 0.15
B) 430
C) 2.4
D) 4.8
E) 4.3

D) 4.8

The internal energy of a system is always increased by __________. A) adding heat to the system B) having the system do work on the surroundings C) withdrawing heat from the system D) adding heat to the system and having the system do work on the surroundings E) a volume compressionA) adding heat to the systemThe value of ΔE for a system that performs 111 kJ of work on its surroundings and gains 89 kJ of heat is __________ kJ. A) -111 B) -200 C) 200 D) -22 E) 22D) -22Of the following, which one is a state function? A) H B) q C) w D) heat E) none of the aboveA) HThe reaction 4Al (s) + 3O2 (g) → 2 Al2O3 (s) ΔH° = -3351 kJ is __________, and therefore heat is __________ by the reaction. A) endothermic, released B) endothermic, absorbed C) exothermic, released D) exothermic, absorbed E) thermoneutral, neither released nor absorbedC) exothermic, releasedThe temperature of a 12.58 g sample of calcium carbonate [CaCO3 (s)] increases from 23.6 °C to 38.2 °C. If the specific heat of calcium carbonate is 0.82 J/g-K, how many joules of heat are absorbed? A) 0.82 B) 5.0 C) 7.5 D) 410 E) 151E) 151For the species in the reaction below, ΔHf° is zero for __________. 2Co (s) + H2 (g) + 8PF3 (g) → 2HCo(PF3)4 (l) A) Co (s) B) H2 (g) C) PF3 (g) D) HCo(PF3)4 (l) E) both Co(s) and H2 (g)E) both Co(s) and H2 (g)Calculate the kinetic energy in J of an electron moving at 6.00 × 106 m/s. The mass of an electron is 9.11 × 10-28 g. A) 4.98 × 10-48 B) 3.28 × 10-14 C) 1.64 × 10-17 D) 2.49 × 10-48 E) 6.56 × 10-14C) 1.64 × 10-17The value of ΔH° for the reaction below is -72 kJ. __________ kJ of heat are released when 80.9 grams of HBr is formed in this reaction. H2 (g) + Br2 (g) → 2HBr (g) A) 144 B) 72 C) 0.44 D) 36 E) -72D) 36The enthalpy change for the following reaction is -483.6 kJ: 2 H2 (g) + O2 (g) → 2 H2O (g) Therefore, the enthalpy change for the following reaction is __________ kJ: 4 H2 (g) + 2 O2 (g) → 4 H2O (g) A) -483.6 B) -967.2 C) 2.34 × 105 D) 483.6 E) 967.2B) -967.2Given the following reactions CaCO3 (s) → CaO (s) + CO2 (g) ΔH = 178.1 kJ C (s, graphite) + O2 (g) → CO2 (g) ΔH = -393.5 kJ the enthalpy of the reaction CaCO3 (s) → CaO (s) + C (s, graphite) + O2 (g) is __________ kJ. A) 215.4 B) 571.6 C) -215.4 D) -571.6 E) 7.01 × 104B) 571.6Given the data in the table below, ΔH°rxn for the reaction Ca(OH)2 + 2 H3AsO4 → Ca(H2AsO4)2 + 2 H2O is __________ kJ. A) -744.9 B) -4519 C) -4219 D) -130.4 E) -76.4C) -4219The wavelength of light emitted from a traffic light having a frequency of 5.75 × 1014 Hz is __________. A) 702 nm B) 641 nm C) 674 nm D) 522 nm E) 583 nmD) 522 nmWhich one of the following is considered to be ionizing radiation? A) visible light B) radio waves C) X-rays D) microwaves E) infrared radiationC) X-raysOf the following transitions in the Bohr hydrogen atom, the __________ transition results in the emission of the highest-energy photon. A) n = 1 → n = 6 B) n = 6 → n = 1 C) n = 6 → n = 3 D) n = 3 → n = 6 E) n = 1 → n = 4B) n = 6 → n = 1The uncertainty principle states that __________. A) matter and energy are really the same thing B) it is impossible to know anything with certainty C) it is impossible to know the exact position and momentum of an electron D) there can only be one uncertain digit in a reported number E) it is impossible to know how many electrons there are in an atomC) it is impossible to know the exact position and momentum of an electronAt maximum, an f-subshell can hold __________ electrons, a d-subshell can hold __________ electrons, and a p-subshell can hold __________ electrons. A) 14, 10, 6 B) 2, 8, 18 C) 14, 8, 2 D) 2, 12, 21 E) 2, 6, 10A) 14, 10, 6Which electron configuration represents a violation of the Pauli exclusion principle?C) 2 up arrows in the same boxThe ground state electron configuration of Fe is __________. A) 1s22s23s23p63d6 B) 1s22s22p63s23p64s23d6 C) 1s22s22p63s23p64s2 D) 1a22s22p63s23p64s24d6 E) 1s22s23s23p10B) 1s22s22p63s23p64s23d6Which electron configuration represents a violation of Hund's rule for an atom in its ground state?B) Skips a boxThe ground state configuration of fluorine is __________. A) [He]2s22p2 B) [He]2s22p3 C) [He]2s22p4 D) [He]2s22p5 E) [He]2s22p6D) [He]2s22p5The energy of a photon of light is __________ proportional to its frequency and __________ proportional to its wavelength. A) directly, directly B) inversely, inversely C) inversely, directly D) directly, inversely E) indirectly, notD) directly, inverselyUsing Bohr's equation for the energy levels of the electron in the hydrogen atom, determine the of an electron in the n = 4 level. A) -1.36 × 10-19 B) -5.45 × 10-19 C) -7.34 × 1018 D) -1.84 × 10-29 E) +1.84 × 10-29A) -1.36 × 10-19The de Broglie wavelength of an electron with a velocity of 6.00 × 106 m/s is __________ m. The mass of the electron is 9.11 × 10-28 g. A) 8.25 × 109 B) 8.25 × 1012 C) 1.21 × 10-16 D) 1.21 × 10-13 E) 1.21 × 10-10E) 1.21 × 10-10The effective nuclear charge of an atom is primarily affected by __________. A) inner electrons B) outer electrons C) nuclear charge D) electron distribution E) orbital radial probabilityA) inner electronsWhich one of the following atoms has the largest radius? A) O B) F C) S D) Cl E) NeC) S__________ is isoelectronic with argon and __________ is isoelectronic with neon. A) Cl-, F- B) Cl-, Cl+ C) F+, F- D) Ne-, Kr+ E) Ne-, Ar+A) Cl-, F-Which equation correctly represents the first ionization of aluminum? A) Al- (g) → Al (g) + e- B) Al (g) → Al- (g) + e- C) Al (g) + e- → Al- (g) D) Al (g) → Al+ (g) + e- E) Al+ (g) + e- → Al (g)D) Al (g) → Al+ (g) + e-Of the elements below, __________ is the most metallic. A) sodium B) barium C) magnesium D) calcium E) cesiumE) cesiumThe list that correctly indicates the order of metallic character is __________. A) B > N > C B) F > Cl > S C) Si > P > S D) P > S > Se E) Na > K > RbC) Si > P > SWhich one of the following elements has an allotrope that is produced in the upper atmosphere by lightning? A) N B) O C) S D) Cl E) HeB) OElements in the modern version of the periodic table are arranged in order of increasing __________. A) oxidation number B) atomic mass C) average atomic mass D) atomic number E) number of isotopesD) atomic numberWhich periodic table group contains only metals? A) 8A B) 2A C) 6A D) 7A E) 5AB) 2AWhich of the following has eight valence electrons? A) Ti4+ B) Kr C) Cl- D) Na+ E) all of the aboveE) all of the aboveThe electron configuration [Kr]4d10 represents __________. A) Sr+2 B) Sn+2 C) Te+2 D) Ag+1 E) Rb+1D) Ag+1Fe+2 ions are represented by __________. A) [Ar]3d1 B) [Ar]3d4 C) [Ar]3d6 D) [Ar]3d104s1 E) [Ar]3d3C) [Ar]3d6In which of the molecules below is the carbon-carbon distance the shortest? A) H2CCH2 B) H-C≡C-H C) H3C-CH3 D) H2CCCH2 E) H3C-CH2-C H3B) H-C≡C-HThe bond length in an HI molecule is 1.61 Å and the measured dipole moment is 0.44 D. What is the magnitude (in units of e) of the negative charge on I in HI? (1 debye = 3.34 × 10-30 coulomb-meters; e=1.6 × 10-19 coulombs) A) 1.6 × 10-19 B) 0.057 C) 9.1 D) 1 E) 0.22B) 0.057In the Lewis symbol for a sulfur atom, there are __________ paired and __________ unpaired electrons. A) 2, 2 B) 4, 2 C) 2, 4 D) 0, 6 E) 5, 1B) 4, 2The Lewis structure of the COH32- ion is __________.A) [O,4 dots double bond. carbon in middle. single bonds with 2 Os 6 dots each]-2To convert from one resonance structure to another, __________. A) only atoms can be moved B) electrons and atoms can both be moved C) only electrons can be moved D) neither electrons nor atoms can be moved E) electrons must be addedC) only electrons can be movedBond enthalpy is __________. A) always positive B) always negative C) sometimes positive, sometimes negative D) always zero E) unpredictableA) always positiveBased on the octet rule, aluminum most likely forms an __________ ion. A) Al3+ B) Al4+ C) Al4- D) Al+ E) Al-A) Al3+The only noble gas without eight valence electrons is __________. A) Ar B) Ne C) He D) Kr E) All noble gases have eight valence electrons.C) HeA __________ covalent bond between the same two atoms is the longest. A) single B) double C) triple D) They are all the same length. E) strongA) singleElectronegativity __________ from left to right within a period and __________ from top to bottom within a group. A) decreases, increases B) increases, increases C) increases, decreases D) stays the same, increases E) increases, stays the sameC) increases, decreasesUsing the table of average bond energies below, the ΔH for the reaction is __________ kJ. Bond: C≡C C-C H-I C-I C-H D (kJ/mol): 839 348 299 240 413 A) +160 B) -160 C) -217 D) -63 E) +63C) -217Using the table of bond dissociation energies, the ΔH for the following reaction is __________ kJ. 2HCl (g) + F2 (g) → 2HF (g) + Cl2 (g) A) -359 B) -223 C) 359 D) 223 E) 208A) -359Of the atoms below, __________ is the most electronegative. A) Si B) Cl C) Rb D) Ca E) SB) Cl

Chem Exam 2

Other sets by this creator

Verified questions

Other Quizlet sets