Chemistry Study GUide
Chemistry Study GUide Chem 111
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This 3 page Study Guide was uploaded by Bailey Wilhoit on Friday September 9, 2016. The Study Guide belongs to Chem 111 at University of South Carolina - Columbia taught by Stefik in Fall 2016. Since its upload, it has received 32 views. For similar materials see Chemsitry in Chemistry at University of South Carolina - Columbia.
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Date Created: 09/09/16
Chemistry Study Guide Exam 1 Ch 1 1. What is chemistry? 2. Explain the differences between law, theory, and hypothesis. 3. Determine if whether these reactions are physical/chemical changes. a. Rusting b. Freezing c. Color change d. Melting 4. Determine whether these properties are chemical or physical, extensive or intensive. a. Water’s Density b. Mass c. Color d. Melting point e. Combustibility f. Methane burning in air 5. What is the difference between a heterogenous mixture and a homogenous mixture? 6. Explain the difference between precision and accuracy. 7. Determine how many significant figures are in each example: a. 0.0098 b. 204.6 c. 650,000 d. 500.0 e. 0.05604 8. Complete the operations with the correct significant figures. a. 54.0634.9 b. 43 x 76.8 c. (12387)x(10+3) 9. Covert 400 L to mL Ch 2 1. What is the law of conservation of mass? 2. What is the law of multiple proportions? 3. T/F a. Electrons are positively charged. b. The amount of electrons and neutrons are the same to balance out the charge. c. Electrons have little to no effect on the mass of an element. d. The atomic number is the sum of the protons and neutrons in an element. e. Isotopes differ in the number of electrons in the nucleus. f. Cations have lost electrons. 10. Write the symbol for the ion with 8 protons, 9 neutrons, and 10 electrons. 11. Groups 1A8A are called: 12. Groups 1B8B are called: 13. Calculate the molecular mass of this compound: a. C O4 5 14. Write the empirical formula of the compound with the cation of Na and the anion of F. 15. List the 7 polyatomic ions you were supposed to memorize: 16. Name these compounds a. NH Br4 b. MnSO 4 17. Write out the name of these acids: a. HCl b. HCN c. HBr 18. Name these compounds: a. N O2 5 b. SCl 5 19. What is the equation for 2 bromopentane? Butane? Ch. 3 1. Balance this equation: a. C H7 2O → 2 + H 2 2 b. What type of reaction is this? 2. Write the equation for sodium nitrate dissolving in water. 3. How many atoms are present in 1.44 mol Mg? 4. How many molecules are in 99.2 mol H O? 2 5. Give the molar mass for N O . 2 4 6. Calculate the mass (in grams) of 3.50 mol NO . 2 7. Determine the oxidation numbers for each: a. CO 2 b. SF 6 c. HNO 3 8. How many moles are in 0.35 mol Na? 9. What is the mass of 0.25 moles of methane CH ? 4 10. How many moles of ethylene, C H ? 2 4 11. What is the mass percentage of each element in C H ? 6 12 12. Calculate the mass of H in 4.33g H O? 2 13. When a 2.074 sample that contains only C, H, and O burns in excess 0 , the products 2 are 3.80g CO and2.04g H O. What i2the empirical formula of this compound? 14. What is the molecular formula for a compound that has an empirical formula C H O and 2 4 a molar mass of 132 g/mol. 15. What is the theoretical yield (in grams) of CO formed from the reaction of 3.12 g CS 2 2 and 1.88 g O ? T2 second product is SO ? 2 16. There is 75.0g NO and 45.0g O . What is th2limiting reactant? Chapter 4 1. Identify whether these compounds dissolve in water: a. BaI 2 b. Lead (II) chloride c. Na CO 2 3 d. Ammonium sulfate 1) Write the net ionic equation for this reaction: a) Solutions of ammonium carbonate and magnesium 2. What are the characteristics of strong and weak electrolytes? 3. Predict the solubility of ammonium carbonate. 4. Write the overall equation, ionic equation, and the net ionic equation for the reaction that occurs when aqueous solutions of lead (II) acetate and barium bromide are mixed. 5 .Calculate the molarity of KOH in a solution prepared by dissolving 8.23 g KOH in enough water to form 250 mL solution. 6.What mass of sodium hydroxide, in grams, is needed to react with 100.0 mL of 3.13 M H2O 4 7. What is the molar concentration of a solution of HNO if 50.00 mL react completely with 22.40 mL of a 0.0229 M solution of Sr(OH) ? 2 8. What volume of 0.223 M HNO is3equired to neutralize 50.00 mL of 0.033 M hydroxide?
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