Give the oxidation number of the underlined atoms in the following molecules

Give the oxidation number of the underlined atoms in

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Give the oxidation number of the underlined atoms in the following molecules and ions: (7 points) a. Cl F 1+ b. I F 7 7+ c. C H 4 4- d. C 2 H 2 1- e. C 2 H 4 2- f. K 2 Cr O 4 6+ g. K 2 Cr 2 O 7 6+ h. KMn O 4 7+ i. NaHC O 3 4+ j. O 2 0 k. NaI O 3 5+ l. K 2 O 2- m. P F 6- 6+ n. Au Cl 4 - 4+ (Reference: Chang 4.47) 5. For the following reactions, identify the type (combination, combustion, decomposition, displacement, methathesis [double-displacement)] neutralization), balance the reaction, and for the redox reactions identify the oxidizing agent and reducing agent. (12 points) (a ) CH 4 + 2O 2 CO 2 + 2H 2 O Combustion, CH4 is reducing agent ,O2 is oxidizing agent (b) HCl + NaOH H 2 O + NaCl Neutralization (c) 2H 2 + O 2 2H 2 O Redox reaction, H2 is the reducing agent O2 is oxidizing agent (d) CaCO 3 + 2HCl CaCl 2 + CO 2 + H 2 O Methathesis 2 Copyright © 2017 by Thomas Edison State University . All rights reserved.
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(e) Zn + 2HCl ZnCl 2 + H 2 Displacement Zn is reducing agent HCL is oxidizing agent (f) 2NaCl 2Na + Cl 2 Decomposition 6. Calculate the molarity of each of the following solutions: (4 points) a. 29.0 g of ethanol (C 2 H 5 OH) in 545 mL of solution b. 9.00 g of sodium chloride (NaCl) in 86.4 mL of solution (Reference: Chang 4.65) a. MOLARITY = MOLES OF SOLUTE/ LITERS OF SOLUTION 29g C2H5OH/ 46.066 C2H5OH = .630 M C2H5OH .630/ .545 = 1.156 M b. 9/58.436 NaCl = .154 .154/.0864= 1.78 M 8. Calculate the mass of KI in grams required to prepare 5.00 × 10 2 mL of a 2.80 M solution. (3 points) 500 ml = .5L 2.8/2 = 1.4 x 165.998 = 232.4 g KI (Reference: Chang 4.59)
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