ex2spring20081045f1

ex2spring20081045f1 - Exam...

Info iconThis preview shows page 1. Sign up to view the full content.

View Full Document Right Arrow Icon
This is the end of the preview. Sign up to access the rest of the document.

Unformatted text preview: Exam Name___________________________________ Form I MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) Consider the following reaction. How many moles of oxygen are required to produce 2.33 moles of water? Assume that there is excess C 3 H7 SH present. C3 H7 SH(l) + 6 O2 (g) → 3 CO 2 (g) + SO2 (g) + 4 H 2 O (g) A) 2.33 moles O 2 B) 3.50 moles O 2 C) 1.55 moles O 2 D) 4.14 moles O 2 E) 6.21 moles O 2 2) Consider the following balanced reaction. What mass (in g) of CO 2 can be formed from 288 mg of O2 ? Assume that there is excess C 3 H7 SH present. C3 H7 SH(l) + 6 O2 (g) → 3 CO 2 (g) + SO2 (g) + 4 H2 O (g) A) 0.198 g CO 2 B) 0.396 g CO 2 C) 0.792 g CO 2 D) 0.209 g CO 2 E) 0.126 g CO 2 3) How many molecules of HCl are formed when 50.0 g of water reacts according to the following balanced reaction? Assume excess ICl3 . 2 ICl3 + 3 H 2 O → ICl + HIO 3 + 5 HCl A) 1.67 × 1024 molecules HCl B) 5.02 × 1025 molecules HCl C) 6.09 × 1025 molecules HCl D) 3.65 × 1024 molecules HCl E) 2.78 × 1024 molecules HCl 3) 2) 1) A‐1 Form I 4) Determine the theoretical yield of H 2 S (in moles) if 4.0 mol Al 2 S3 and 4.0 mol H 2 O are reacted according to the following balanced reaction. A possibly useful molar mass is Al 2 S3 = 150.17 g/mol. Al2 S3 (s) + 6 H2 O(l) → 2 Al(OH)3 (s) + 3 H 2 S(g) A) 12 mol H2 S B) 2.0 mol H2 S C) 4.0 mol H2 S D) 6.0 mol H2 S E) 18 mol H2 S 5) How many milliliters of a 0.184 M NaNO 3 solution contain 0.113 moles of NaNO 3 ? A) 614 mL B) 885 mL C) 326 mL D) 163 mL E) 543 mL 4) 5) 6) Which of the following is considered a STRONG electrolyte? A) C12H22O11 B) CH3 OH C) HC2 H3 O2 D) NH4 NO3 E) PbCl2 7) Which of the following pairs of aqueous solutions will react when mixed? A) AgC 2 H3 O2 + Cu(NO 3 )2 B) NaCl + Li3 PO4 C) Hg2 (NO3 )2 + LiI D) NH4 NO3 + Li2 CO 3 E) None of the above solution pairs will produce a reaction. 8) Give the net ionic equation for the reaction (if any) that occurs when aqueous solutions of H 2 SO4 and KOH are mixed. A) H2 2+(aq) + OH- (aq) → H2 (OH)2 (l) B) H+ (aq) + OH- (aq) → H2 O(l) C) 2 K+ (aq) + SO 4 2 - (aq) → K2 SO4 (s) D) H+ (aq) + OH- (aq) + 2 K+ (aq) + SO4 2 - (aq) → H2 O(l) + K2 SO4 (s) E) No reaction occurs. 6) 7) 8) A‐2 Form I 9) Identify the spectator ions in the following molecular equation. KBr(aq) + AgNO 3 (aq) → AgBr(s) + KNO 3 (aq) A) Ag+ & NO3 B) K+ & NO3 C) K+ & BrD) Ag+ & BrE) There are no spectator ions in this reaction. 10) Determine the oxidation state of P in PO3 3 - . A) +6 B) - 3 C) +2 D) 0 E) +3 9) 10) 11) Determine the oxidizing agent in the following reaction. Ni(s) + 2 AgClO4 (aq) → Ni(ClO4 )2 (aq) + 2 Ag(s) A) O B) Ni C) Ag D) Cl E) This is not an oxidation- reduction reaction. 12) Determine the number of grams H2 formed when 250.0 mL of 0.743 M HCl solution reacts with 3.41 x 1023 atoms of Fe according to the following reaction. 2 HCl(aq) + Fe(s) → H2 (g) + FeCl 2 (aq) A) 0.374 g B) 0.187 g C) 1.33 g D) 1.14 g E) 1.51 g 11) 12) 13) Calculate the frequency of the red light emitted by a neon sign with a wavelength of 659.9 nm. A) 1.98 × 1014 s - 1 B) 5.05 × 1014 s - 1 C) 2.20 × 1014 s - 1 D) 3.32 × 1014 s - 1 E) 4.55 × 1014 s - 1 14) Each of the following sets of quantum numbers is supposed to specify an orbital. Which of the following sets of quantum numbers contains an error? A) n = 3, l =3 , ml = - 2 B) n = 1, l = 0, ml =0 C) n = 4, l = 2, ml =0 D) n = 2, l = 1 , ml = - 1 E) n = 3, l = 0, ml =0 15) How many orbitals are contained in the third principal level ( n=3) of a given atom? A) 7 B) 9 C) 5 D) 3 A‐3 13) 14) 15) E) 18 Form I 16) In which orbital below would an electron (on average) be closest to the nucleus? A) 4s B) 3p C) 5d D) 2s 17) Give the ground state electron configuration for I. A) [Kr]5s2 4d 105p5 B) [Kr]4d105p6 C) [Kr]5s2 4d 105p6 D) [Kr]5s2 5p6 E) [Kr]5s2 5d 105p6 18) Give the ground state electron configuration for Mg2 ⁺. A) 1s2 2s2 2p6 3s2 3p6 B) 1s2 2s2 2p6 3s2 C) 1s2 2s2 2p6 D) 1s2 2s2 2p6 3s2 3p2 E) 1s2 2s2 2p6 3s1 19) Choose the ground state electron configuration for Cr 3 ⁺. A) [Ar]4s2 3d 1 B) [Ar]4s2 3d 6 C) [Ar]3d3 D) [Ar] E) [Ar]4s1 3d 2 16) E) 2p 17) 18) 19) 20) Give the set of four quantum numbers that represent the last electron added (using the Aufbau principle) to the Zn atom. 1 A) n = 3, l = 3, ml = 2, ms = - 2 B) n = 3, l = 2, ml = 0, ms = + C) n = 4, l = 3, ml = 3, ms = - D) n = 3, l = 2, ml = 2, ms = - E) n = 3, l = 1, ml = 1, ms = + 1 2 1 2 1 2 1 2 20) 21) How many of the following species are paramagnetic? Sc3 ⁺ A) 1 Br⁻ B) 3 Mg 2 ⁺ Se C) 2 D) 0 E) 4 21) A‐4 Form I 22) Place the following in order of increasing atomic radius. As A) Br < As < O B) As < O < Br C) O < As < Br D) As < Br < O E) O < Br < As 23) Place the following in order of increasing IE1 . N A) As < N < F B) F < N < As C) F < N < As D) As < F < N E) N < As < F 24) How many valence electrons does an atom of S have? A) 3 B) 4 C) 2 25) The form number designated at the top of my exam is A) form I B) form II C) form III F As O Br 22) 23) 24) D) 6 E) 1 25) D) form IV E) form V A‐5 Answer Key Testname: EX2SPRING20081045 1) B 2) A 3) E 4) B 5) A 6) D 7) C 8) B 9) B 10) E 11) C 12) B 13) E 14) A 15) B 16) D 17) A 18) C 19) C 20) D any answer accepted 21) A 22) E 23) A 24) D 25) No Correct Answer Was Provided. A‐6 ...
View Full Document

Ask a homework question - tutors are online