CHEM 1311 - Test 1 Practice Questions
CHEM 1311 - Test 1 Practice Questions CHEM1311
Austin Community College
Popular in General Chemistry I
Popular in Chemistry
This 7 page Study Guide was uploaded by Cindy Trinh on Monday September 26, 2016. The Study Guide belongs to CHEM1311 at Austin Community College taught by Elisa Cooper in Winter2015. Since its upload, it has received 6 views. For similar materials see General Chemistry I in Chemistry at Austin Community College.
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Date Created: 09/26/16
- OH - 3 NO 34 PO 2- 3 CO - CN 3- P 2- O - Cl + 4 3+ 2+ + 4+ 3+ + 2+ Al Ni Ag Sn Fe NH K Ca Practice problems for exam 1: 1. Briefly explain the difference between covalent and ionic bonds. 2. List all of the covalent compounds represented in the following equation NH 3 + CuO → Cu + N2 + H 2 3. In parts a and b, identify each of the compounds as ionic or covalent and give the correct chemical name. In parts c and d, give the formula that would result between the two given elements or ions and the correct chemical name. a) N 2 4 b) Fe(OH) 3 c) Sodium and Sulfur 2+ 3- d) Ca and PO 4 4. Venus, the second planet from the sun, has a surface temperature of 7.3 x 10 K. Convert this temperature t°C and °F. 5. The average speed of an atom of helium at 25 °C is 1255 m/s. Convert this speed to miles per hour. (1 mile = 1.609 km) 3 6. Aspirin has a density of 1.40 g/cm . What is the volume (in cubic centimeters) of an aspirin tablet weighing 385 mg? 7. A 125 mL sample of water initially at 293.2 K was heated for 8 minutes. Over this time period, the temperature of the water rose at a constant rate of 3.0 °F/min. What is the final temperature of the water in degrees Fahrenheit? 8. Consider the as yet undiscovered elements with atomic numbers 115, 117 and 119. a) Which element would be a halogen? b) Which element should have chemical properties similar to cesium (Cs)? c) If an ion of element 115 was found to have a charge of -3, how many protons and electrons would the ion have? d) If an atom of element 119 was found to have a mass of 296 atomic mass units, how many protons, electrons and neutrons would this atom have? Write the standard isotopic symbol for this atom using Ec as the symbol for this element. 9. Classify each of the following properties as chemical or physical AND intrinsic or extrinsic a) The scent of a lemon b) The mass of an orange c) The boiling point of ethyl alcohol d) Silver becomes tarnished after exposure to air for a long period of time 10. Identify each of the following as an element, atom, molecule or compound. More than one term may apply to any given formula. List all terms that apply for each a) Br2 b) Rb(OH) 2 c) C 3 5 O3 9 d) S8 11. Identify each of the compounds as ionic or covalent and give the correct chemical name. a) K 2 b) N 2O c) FeS d) S2O 3 e) H SO 2 4 f) HNO 2 12. Write the correct formula for the given name. a) Sulfur trioxide b) Calcium sulfate c) Lithium oxide d) Manganese(III) hydroxide e) ammonium carbonate 13. Provide two acceptable names for HF. 14. Monosodium glutamate (MSG), a food-flavor enhancer, has been blamed for “Chinese restaurant syndrome,” the symptoms of which are headaches and chest pains. MSG has the following composition by mass: 35.51 percent C, 4.77 percent H, 37.85 percent O, 8.29 percent N and 13.60 percent Na. What is its molecular formula if its molar mass is about 169 g/mol? 15. Vitamin C (ascorbic acid) contains only C, H and O. Vitamin C is 40.92% C and 4.58% H. Determine the empirical formula of vitamin C. 16. How many atoms are in 6.28 g of Al? 17. How many moles are in 12.4 g of He? 18. How many moles are in 1.95 mg of Fe(OH) ? Ho3 many atoms of oxygen are contained in 1.95 mg of Fe(OH) ? 3 19. How many atoms are in 12.8 g of CCl ? 4 20. What is the mass (in grams) of 1.57 x 10 molecules of water? 21. Calculate the molar mass of glucose and ethanol. Glucose: C 6H 12 6 Ethanol: C 2 O5 22. The average U.S. farm occupies 435 acres. How many square miles is this? 2 1 acre = 43,560 ft , 1 mile = 5280 ft 23. Uranium-235 is used in nuclear fission. Determine the number of protons and neutrons in uranium-235 and give the standard isotopic symbol. 21 24. What is the mass in grams of 4.92×10 platinum (Pt) atoms? 25. When iron rusts, solid iron reacts with gaseous oxygen to form solid iron(III) oxide. Write a balanced chemical equation for this reaction. 26. Write a balanced chemical equation for the following reactions: a) Sulfur dioxide gas reacts with oxygen gas to form sulfur trioxide gas. b) Gaseous ammonia (NH 3) reacts with gaseous oxygen to for gaseous nitrogen monoxide and gaseous water. 27. A drop of water has a volume of approximately 0.05 mL. How many water molecules does it contain? The density of water is 1.0 g/cm 3. 1 mL = 1 cm 3 28. What mass of electrons are needed to have a charge of -1.0 Coulombs? 29. How many atoms of oxygen are in 1.5 g of Mg(ClO) 2? 30. Balance the following equation: C H (g) + O (g) → CO (g) + H O (g) 4 10 2 2 2 31. Balance the following equation and name each of the compounds: Na 2 (aq) + Cu(NO )3 2q) → NaNO (3q) + CuS (s) 32. Write a balanced chemical equation for the following: Aqueous hydrochloric acid reacts with solid manganese (IV) oxide to form aqueous manganese (II) chloride, liquid water and chlorine gas. 33. Determine the number of protons, neutrons and electrons in each of the following species: a) An atom of Ca-40 b) The ion formed from a bromine-79 atom c) An ion of Al-27 with a charge of +3 d) 18Ta 73 34. Write the formula that would result between the two given elements or ions: a) Na and PO 3- + 2- b) NH 4 and S c) The ionic compound formed between sulfur and calcium Name each of the following acids: d) H 2O 4 e) HI Determine if each of the following compounds is covalent or ionic and provide the correct chemical name for each: f) H 3O 4 g) PCl 5 h) Mg(OH) 2 35. Analysis of a metal chloride XCl s3ows that it contains 67.2% Cl by mass. Calculate the molar mass of X and identify the element. 36. Traumatic acid is a compound of carbon, hydrogen and oxygen and is a plant hormone which causes injured cells to divide and help repair the trauma. Combustion analysis of a 1.52 g sample of traumatic acid produced 1.200 g of water and 3.516 g of carbon dioxide. Determine the empirical formula of traumatic acid. 1. Covalent bonds result from the sharing of electrons between two atoms. Ionic bonds result from the transfer of electrons between two atoms. 2. NH a3d H O 2 3. a. Dinitrogen tetroxide, covalent b. Iron (III) hydroxide, ionic c. Na 2, sodium sulfide d. Ca 3PO )4 2calcium phosphate 4. 460 °C, 850 °F 5. 2808 mi/hr 6. 0.275 cm 3 7. 92.1 °F 8. a. 117 b. 119 - c. p = 115, e = 118 d. p = 119, e = 119, n = 177 296 Ec 119 9. a. Physical, intrinsic b. Physical, extrinsic c. Physical, intrinsic d. Chemical, intrinsic 10. a. Element, molecule b. compound c. Compound, molecule d. Element, molecule 11. a. ionic, potassium oxide b. covalent, dinitrogen monoxide c. ionic, iron (II) sulfide d. covalent, disulfur trioxide e. covalent, sulfuric acid f. covalent, nitrous acid 12. a. SO 3 b. CaSO 4 c. Li O 2 d. Mn(OH) 3 e. (NH )4 2 3 13. hydrogen fluoride and hydrofluoric acid 14. C 5 8 N4a 15. C 3 4 3 23 16. 1.40 x 10 atoms 17. 3.10 moles 18. 1.82 x 10-5moles, 3.30 x 10 19 atoms of oxygen 23 19. 2.51 x 10 atoms 20. 4.70 x 10 g 21. glucose: 180.16 g/mol, ethanol: 46.07 g/mol 2 22. 0.680 mi 23. 92 p, 143n 235U 92 24. 1.59 25. 4 Fe (s) + 3 O (g) → 2 Fe O (s) 2 2 3 26. a. 2 SO (g) + O (g) → 2 SO (g) 2 2 3 b. 4 NH (g3 + 5 O (g)2→ 4 NO (g) + 6 H O (g) 2 27. 2 x 10 molecules -9 28. 5.7 x 10 g 29. 1.4 x 10 atoms 30. 2 C H4 10(g) + 13 O (2) → 8 CO (2) + 10 H 2 (g) 31. Na 2 (aq) + Cu(NO ) 3 2) → 2 NaNO (a3) + CuS (s) sodium sulfide copper (II) nitrate sodium nitrate copper(II) sulfide 32. 4 HCl (aq) + MnO (s) 2 MnCl (aq) + 22H O (l) + C2 (g) 2 33. a. p = 20, n = 40-20 = 20, e = 20 - b. p = 35, n = 79-35 = 44, e = -6 c. p = 13, n = 27-13 = 14, e = 10 d. p = 73, n = 181-73 = 108, e = 73 34. a. Na P3 4 b. (NH ) 4 2 c. CaS d. Sulfuric acid e. hydroiodic acid f. phosphoric acid (or trihydrogren phosphate), covalent g. phosphorous pentachloride, covalent h. magnesium hydroxide, ionic 35. 51.9 g/mol, Cr 36. C 3H 5
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