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Practice Exam 2 Questions - University Chemistry I | CHEM 1103, Exams of Chemistry

University of Arkansas (UA)Chemistry
Prof. Mya Norman

Material Type: Exam; Professor: Norman; Class: UNIVERSITY CHEM I; Subject: Chemistry; University: University of Arkansas Main Campus;

Typology: Exams

2011/2012

Uploaded on 04/11/2012

shane-germany
shane-germany 🇺🇸

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Practice Exam 2 Spring 2012
1. How many moles of oxygen atoms are there in 1.5 mol of the compound
CuSO4?
A. 5.5 mol
B. 2.5 mol
C. 2.0 mol
D. 6.0 mol
E. 1.0 mol
2. Which of the following has the greatest mass?
A. 75 mL water (d = 1 g/mL)
B. 0.62 mol sucrose (C6H12O6)
C. 2.65 x 1025 P atoms
D. 1.25 mol Oxygen molecules
E. 44.3 g Al2O3
3. Calculate the number of atoms in 10.0 g CO2
A. 1.37x1023
B. 3.83x1018
C. 2.41x1024
D. 4.10 x1023
E. 6.02x1024
4. How many molecules of ethanol (CH3CH2OH) are present in 42.4 mL of Ethanol if it has a
density of 0.789 g/mL?
A. 7.024 x 1023
B. 9.28 x 1026
C. 5.16 x 1023
D. 8.30 x 1023
E. 4.38x1023
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Download Practice Exam 2 Questions - University Chemistry I | CHEM 1103 and more Exams Chemistry in PDF only on Docsity!

Practice Exam 2 Spring 2012

  1. How many moles of oxygen atoms are there in 1.5 mol of the compound CuSO 4? A. 5.5 mol B. 2.5 mol C. 2.0 mol D. 6.0 mol E. 1.0 mol
  2. Which of the following has the greatest mass? A. 75 mL water (d = 1 g/mL) B. 0.62 mol sucrose (C 6 H 12 O 6 ) C. 2.65 x 10^25 P atoms D. 1.25 mol Oxygen molecules E. 44.3 g Al 2 O 3
  3. Calculate the number of atoms in 10.0 g CO 2 A. 1.37x10^23 B. 3.83x10^18 C. 2.41x10^24 D. 4.10 x10^23 E. 6.02x10^24
  4. How many molecules of ethanol (CH 3 CH 2 OH) are present in 42.4 mL of Ethanol if it has a density of 0.789 g/mL? A. 7.024 x 10^23 B. 9.28 x 10^26 C. 5.16 x 10^23 D. 8.30 x 10^23 E. 4.38x10^23
  1. How many moles of Ba2+^ ions are there in 2.25 moles of barium sulfate? A. 1. B. 2. C. 137 D. 1. E. 4.
  2. How many moles of sodium phosphate are there in 5.7g of sodium phosphate? A. 0.035 mol B. 28.8 mol C. 935 mol D. 2.1 × 10^22 mol E. 1.24 mol
  3. How many hydrogen atoms are in 15 g of ethanol (CH 3 CH 2 OH)? A. 75 B. 1.96 x 10^23 C. 1.18 x 10^24 D. 0. E. 6.02 x 10^23
  4. Limestone (CaCO 3 ) reacts with hydrochloric acid according to the equation CaCO 3 + 2 HCl --> CaCl 2 + H 2 O+CO 2. How many moles of CO 2 gas can be formed by the reaction of 2.35g of CaCO 3 with excess HCl? A. 2.35 x 10- B. 3.22 x 10- C. 0. D. 7.76 x 10- E. 6.44 x 10-
  5. What is the mass of 0.0030 mol of Valium (C 16 H 13 ClN 2 O) in grams? A. 0.856 g B. 8.56 g C. 429 g D. 21.9 g E. 16.
  1. Limestone (CaCO 3 ) reacts with hydrochloric acid according to the equation CaCO 3 + 2 HCl --> CaCl 2 + H 2 O+CO 2. How many moles of CO 2 gas can be formed by the reaction of 2.35g of CaCO 3 with 2.35g HCl? A. 2.35 x 10- B. 3.22 x 10- C. 0. D. 7.76 x 10- E. 6.44 x 10-
  2. Citric acid (C 6 H 8 O 7 ) is prepared industrially via the fermentation of sucrose (C 12 H 22 O 11 ) according to the chemical equation: C 12 H 22 O 11 + H 2 O + 3O 2  2C 6 H 8 O 7 + 4H 2 O If the yield of citric acid is 92.3 %, what is the mass of citric acid produced from 1 metric ton (1 × 106 g) of sucrose? The molar mass of C 12 H 22 O 11 is 342.3 g/mol and the molar mass of C 6 H 8 O 7 is 192 g/mol. A. 1035 kg B. 1000 kg C. 923 kg D. 393 kg E. 518 kg
  3. When 0.024mol of sodium sulfate was dissolved in 500mL water, what is the concentration of Na+^ in the resulting solution? A. 0.060 M B. 0.096 M C. 0.048 M D. 0.144 M E. 0.024 M
  1. Write the total ionic equation for the reaction of dilute BaCl 2 (aq) with Fe 2 (SO 4 ) 3 (aq). What are the spectator ions in this reaction? A. Fe3+^ and Cl– B. Ba2+^ and SO 4 2– C. Fe3+, Cl–, Ba2+^ and SO 4 2– D. There are no spectator ions for this reaction. E. Fe3+^ and Ba2+
  2. Mixing 200 ml of a 0.20M KOH(aq) with excess MgCl 2 will yield which solid of the following during a precipitation reaction? A. 0.080 moles of Mg(OH) 2 B. 0.020 moles of Mg(OH) 2 C. 0.040 moles of KCl D. 0.040 moles of Mg(OH) 2 E. 0.080 moles of KCl
  3. If 42.45 mL of HCl is required to neutralize completely 1.050 g Na 2 CO 3 , what is the molarity of the HCl? The products are NaCl, CO 2 , and H 2 O. Molar mass of Na 2 CO 3 is 106.0 g/mol. A. 0.9334 M B. 1.468 M C. 0.4667 M D. 0.2333 M E. 0.2530 M
  4. The first step in an analysis of water for dissolved oxygen involves the reaction 4 Mn(OH) 2 (aq) + O 2 (aq) + 2 H 2 O(aq)  4 Mn(OH) 3 (s) If appropriate treatment of 4.000 L of water from a creek produces 0.303 g of Mn(OH) 3 , how many grams of O 2 (aq) does that 4L sample of the water contain? The molecular weight of Mn(OH) 3 is 105.94 g/mol. A. 32.1 g B. 0.124 g C. 0.0229 g D. 0.0915g E. 0.873 g
  1. If 5.0 grams of NO and 5.0 grams of Cl 2 react to produce NOCl 2 according to the equation below and the reaction goes to completion, what is the limiting reagent and how many grams of the excess reagent remain at the end of the reaction? Use the reaction: NO + Cl 2NOCl 2 a) NO limits and 1.80 g of Cl 2 remain b) Cl 2 limits and 1.83 g of NO remain c) NO limits and 2.11 g of Cl 2 remain d) Cl 2 limits and 2.89 g of NO remain
  2. KO 2 reacts with CO 2 as shown in the balanced equation below. Calculate the amount of oxygen gas that can be produced when 2.50 g of KO 2 and 4.50 g of CO 2 react. 4 KO 2 (s) + 2 CO 2 (g)2 K 2 CO 3 (s) + 3 O 2 (g) a) 0.422 g b) 1.13 g c) 0.844 g d) 4.90 g e) 1.50 g
  3. A mass of 11.60 g of phosphoric acid was produced from the reaction of 10.00 grams of P 4 O 10 with 12.0 grams of water. What was the % yield for this reaction? The molar mass of P 4 O 10 = 283.88 grams/mole and the molar mass of H 3 PO 4 = 98.00 grams/mole. a) 56.0% b) 84.00% c) 92.70% d) 78.62% e) 101.1%
  4. When 12.6 grams of KBr (molar mass = 119 g/mole) are added to enough water to make 250 ml of solution, what is the molarity of that solution? a) 0.87 M b) 0.28 M c) 0.62 M d) 0.42 M e) 0.53 M
  5. You dissolve 20.00 grams of K 3 PO 4 (molar mass = 212.27 grams/mole) in enough water to make 250.0 ml of solution. What is the [K+] in this solution? a) 0.597 M b) 1.13 M c) 0.240 M d) 0.198 M e) 0.377 M
  1. You dissolve 47.8 milligrams of AgNO 2 (molar mass = 153.9 g/mol) in water to make 10. ml of solution. You then take 3.00 ml of that solution and dilute it to make a new solution with a total volume of 1.00 L. What is the concentration of the Ag+^ ion in the final solution? a) 9.32 x 10-5^ M b) 9.32 x 10-3^ M c) 14.34 M d) 1.43 x 10-2^ M