Straighterline CHEM101 General Chemistry I Midterm Exam (New Version June 2024)

Question 1 Correct 4.00 points out of 4.00 The SI base unit of mass is Select one: A. g. B. metric ton. C. mg. D. lb. E. kg. Question 2 Correct 4.00 points out of 4.00 The boiling point for liquid nitrogen is 77 K. What is the temperature in degrees Fahrenheit? Select one: A. –289°F B. –321°F C. –127°F D. 662°F E. 177°F Straighterline CHEM101 General Chemistry I Midterm Exam (New Version June 2024) We are a team of experts offering class attendance for all Straighterline, Online ATI, HESI, NCLEX, Portage Learning, Sophia etc courses (including final proctored exams!!). We also write essays, discussion posts, research papers and school assignments. Should you need any of these services, Contact us via email: or : +1 (540) 753-5914. Guaranteed Passing! CHEM101_MH_V6 | Topic 9: Energy Changes in Chemical Reactions Started on State Finished Completed on Time taken 1 hour 18 mins GradeQuestion 4 Correct 4.00 points out of 4.00 Acetic acid boils at 244.2°F. What is its boiling point in degrees Celsius? Select one: A. 382.0°C B. 103.7°C C. 117.9°C D. 167.7°C E. 153.4°C Question 5 Correct 4.00 points out of 4.00 One of the common intravenous fluids, called physiological saline, is a homogeneous mixture of NaCl in water. In this mixture, 0.89% of the mass is contributed by the NaCl. What mass of NaCl is found in 450. mL of physiological saline? (Density of physiological saline = 1.005 g/cm3) Select one: A. 2.0 g B. 5.1 g C. 4.0 g D. 508 g E. 400 g Question 3 Correct 4.00 points out of 4.00 Which of the following cannot be separated into simpler substances by chemical means? Select one: A. Homogeneous mixture B. Compound C. Element D. Emulsion E. Heterogeneous mixtureQuestion 7 Correct 4.00 points out of 4.00 Which of these materials are typically poor conductors of heat and electricity? Select one: A. Alkaline earth metals B. Metalloids C. Alkali metals D. Nonmetals E. Metals Question 8 Correct 4.00 points out of 4.00 The elements in Group 2 are known by what name? Select one: A. Noble gases B. Halogens C. Alkaline earth metals D. Alkali metals E. Transition metals Question 6 Correct 4.00 points out of 4.00 Which of the following is the empirical formula for hexane, C6H14? Select one: A. C0.43H B. C12H28 C. C6H14 D. C3H7 E. CH2.3Question 10 Correct 4.00 points out of 4.00 What is the formula of iodous acid? Select one: A. HIO3 B. HIO4 C. HIO2 D. HI E. HIO Question 11 Correct 4.00 points out of 4.00 Determine the number of ammonia molecules in 4.85 g of ammonia. (NA = 6.022 × 1023 mol– 1) Select one: A. 5.83 × 10–24 molecules B. 4.73 × 10–25 molecules C. 1.71 × 1023 molecules D. 1.24 × 1023 molecules E. 2.92 × 1023 molecules Question 9 Correct 4.00 points out of 4.00 Which of these pairs of elements would be most likely to form an ionic compound? Select one: A. Al and Rb B. C and O C. P and Br D. Cu and K E. O and ZnQuestion 13 Correct 4.00 points out of 4.00 Calculate the formula mass of rubidium carbonate, Rb2CO3. Select one: A. 230.95 amu B. 145.47 amu C. 255.00 amu D. 113.48 amu E. 340.43 amu Question 14 Correct 4.00 points out of 4.00 Tetraphosphorus hexoxide is formed by the reaction of phosphorus with oxygen gas. If a mixture of 75.3 g of phosphorus and 38.7 g of oxygen produce 43.3 g of P4O6, what is the percent yield for the reaction? Select one: A. 89.4% B. 57.5% C. 38.0% D. 16.3% E. 48.8% Question 12 Correct 4.00 points out of 4.00 Once the following equation is balanced with the smallest set of whole number coefficients, what is the sum of the coefficients? (Don't forget to include coefficients of one.) Al + H2SO4 → Al2(SO4)3 + _________H2 Select one: A. 12 B. 9 C. 5 D. 3 E. 6Question 16 Correct 4.00 points out of 4.00 Lead(II) sulfide was once used in glazing earthenware. It will also react with hydrogen peroxide to form lead(II) sulfate and water. How many grams of hydrogen peroxide are needed to react completely with 265 g of lead(II) sulfide? Select one: A. 151 g B. 9.41 g C. 123 g D. 50.3 g E. 37.7 g Question 15 Correct 4.00 points out of 4.00 What mass of nitrogen gas is required to react completely with excess hydrogen gas to produce 13.6 g of ammonia? Select one: A. 11.2 g B. 44.8 g C. 0.06 g D. 22.4 g E. 16.5 gQuestion 17 Correct 4.00 points out of 4.00 Using Hess's law, what is ΔH°rxn for the following reaction? WO3(s) + 3H2(g) → W(s) + 3H2O(g) 2W(s) + 3O2(g) → 2WO3(s) 2H2(g) + O2(g) → 2H2O(g) ΔH° rxn = –1685.8 kJ/mol ΔH° rxn = –483.6 kJ/mol Select one: A. 117.5 kJ/mol B. 235.0 kJ/mol C. 1202.2 kJ/mol D. 359.3 kJ/mol E. 2169.4 kJ/molSuppose a 0.500-g sample of an organic compound is analyzed via bomb calorimetry. The temperature of the calorimeter is measured over time. At t = 5 min, the combustion reaction is initiated. Below is a plot of the data that are obtained. Suppose the experiment is repeated under identical conditions, but with a 1.000-g sample of the organic compound. What might a plot of the resulting data look like? Select one: A. Question 18 Incorrect 0.00 points out of 4.00B. C.D. E.Question 20 Correct 4.00 points out of 4.00 The dissolution of barium hydroxide in water is an exothermic process. Which statement is correct? Select one: A. When barium hydroxide dissolves in water, the system does work on the surroundings. B. The temperature of the solution is lower than of the barium hydroxide and water before mixing. C. The enthalpy of solid barium hydroxide plus pure water is less than that of the solution, at the same temperature. D. The enthalpy of solid barium hydroxide plus pure water is the same as that of the solution, at the same temperature. E. The enthalpy of solid barium hydroxide plus pure water is greater than that of the solution, at the same temperature. Question 19 Correct 4.00 points out of 4.00 Suppose a 50-g block of silver (specific heat = 0.2350 J/g·°C) at 100°C is placed in contact with a 50-g block of iron (specific heat = 0.4494 J/g·°C) at 0°C, and the two blocks are insulated from the rest of the universe. The final temperature of the two blocks Select one: A. will be lower than 50°C. B. will be higher than 50°C. C. will be exactly 50°C. D. is unrelated to the composition of the blocks. E. cannot be predicted.Question 22 Correct 4.00 points out of 4.00 The specific heat (capacity) is Select one: A. the amount of energy needed to increase the temperature of 1 mol of a substance by 1°C. B. the amount of energy needed to increase the temperature of 1 g of a substance by 1°C. C. the temperature increase, in K, associated with heating 1 g of a substance for 1 minute. D. the amount of energy required to melt 1 g of substance. E. the amount of substance that is heated by 1°C. Question 21 Correct 4.00 points out of 4.00 What is ΔH° rxn for the decomposition of calcium carbonate to calcium oxide and carbon dioxide? CaCO3(s) → CaO(s) + CO2(g) Substance CaCO3(s) CaO(s) CO2(g) (kJ/mol) –1206.9 –635.6 –393.5 Select one: A. –2236.0 kJ/mol B. 177.8 kJ/mol C. –1449.0 kJ/mol D. 2236.0 kJ/mol E. –177.8 kJ/molQuestion 24 Correct 4.00 points out of 4.00 De Broglie explained electron movements by relating them to Select one: A. waves only. B. waves and particles. C. particles only. D. None of these choices is correct. Question 25 Correct 4.00 points out of 4.00 What is the maximum number of electrons in an atom that can have the following set of quantum numbers? n = 4, l = 3, ml = –2, ms = +1/2 Select one: A. 6 B. 10 C. 2 D. 1 E. 0 Question 23 Correct 4.00 points out of 4.00 A neutral atom in its ground state contains 28 electrons. This element is considered a element, and has electrons in orbitals with l = 2. Select one: A. actinide, 10 B. transition, 8 C. main group, 10 D. main group, 8 E. transition, 10Which one of the following sets of quantum numbers is not possible? Select one: A. A B. B C. C D. D E. E Question 26 Incorrect Question 27 Correct 4.00 points out of 4.00 Calculate the de Broglie wavelength of a neutron that has a velocity of 200. cm/s. (mass of a neutron = 1.675 × 10–27 kg and h = 6.63 × 10–34 J • s) Select one: A. 216 nm B. 1.98 × 10–9 m C. 198 nm D. 1.8 × 1050 m E. 5.05 mm 0.00 points out n l ml ms of 4.00 A 4 3 –2 +1/2 B 3 2 –3 –1/2 C 3 0 0 +1/2 D 4 1 1 –1/2 E 2 0 0 +1/2Question 29 Correct 4.00 points out of 4.00 Which of these elements has the greatest metallic character? Select one: A. Se B. Si C. As D. Br E. Ni Question 30 Correct 4.00 points out of 4.00 An element with the electron configuration [noble gas]ns2(n – 1)d8 has valence electrons. Select one: A. 6 B. 8 C. 2 D. 10 E. None of these choices is correct. Question 28 Correct 4.00 points out of 4.00 Which element would be expected to have properties similar to calcium? Select one: A. Na B. Ba C. Sc D. Rb E. KQuestion 32 Correct 4.00 points out of 4.00 Select the element with the least metallic character. Select one: A. Sr B. Sn C. Tl D. Ga E. Ge Question 31 Incorrect 0.00 points out of 4.00 Which of the following elements has the smallest atomic size? Select one: A. Na B. Ca C. Kr D. Ar E. KHydrazine, N2H4, is a good reducing agent that has been used as a component in rocket fuels. Select its Lewis structure. Select one: A. B. C. D. E. None of the choices is correct. Question 33 Incorrect 0.00 points out of 4.00Question 35 Correct 4.00 points out of 4.00 Select the compound with the lowest (i.e., least negative) lattice energy. Select one: A. KBr(s) B. CsBr(s) C. CaO(s) D. NaCl(s) E. SrO(s) Question 34 Correct 4.00 points out of 4.00 In the following Lewis structure for ClO3F, chlorine has a formal charge of and an oxidation number of . Select one: A. 7, –1 B. 1, –1 C. 7, 7 D. 1, 7 E. 1, 1Question 37 Incorrect 0.00 points out of 4.00 If an element is bonded to 4 other atoms and has a formal charge of +1, what group must the element be in? Select one: A. 17 B. 13 C. 14 D. 15 E. 16 Question 38 Incorrect 0.00 points out of 4.00 According to the VSEPR model, a molecule with the general formula AB4 with two lone pairs on the central atom will have a(n) molecular geometry. Select one: A. seesaw B. square planar C. square pyramidal D. tetrahedral E. octahedral Question 36 Incorrect 0.00 points out of 4.00 The Lewis structure for a chlorate ion, ClO3–, should show single bond(s), double bond(s), and lone pair(s). Select one: A. 3, 0, 10 B. 1, 2, 8 C. 3, 0, 9 D. 1, 2, 7 E. 2, 1, 9Question 40 Incorrect 0.00 points out of 4.00 According to the VSEPR model, the predicted molecular geometry of SiCl4 is Select one: A. bent. B. linear. C. tetrahedral. D. trigonal planar. E. trigonal pyramidal. Question 41 Correct 4.00 points out of 4.00 The nitrosonium ion, NO+, forms a number of interesting complexes with nickel, cobalt, and iron. According to molecular orbital theory, which statement about NO+ is correct? Select one: A. NO+ has a bond order of 3 and is diamagnetic. B. NO+ has a bond order of 2 and is diamagnetic. C. NO+ has a bond order of 2 and is paramagnetic. D. NO+ has a bond order of 2.5 and is neither paramagnetic nor diamagnetic. E. NO+ has a bond order of 3 and is paramagnetic. Question 39 Correct 4.00 points out of 4.00 According to the VSEPR model, which molecule is predicted to have a molecular geometry that is trigonal bipyramidal? Select one: A. SF4 B. XeF4 C. SF6 D. NF3 E. PF5Question 43 Correct 4.00 points out of 4.00 What is the predicted molecular geometry of the H2O molecule according to the VSEPR model? Select one: A. bent B. tetrahedral C. seesaw D. square planar E. trigonal pyramidal Question 44 Correct 4.00 points out of 4.00 Find the pH of a 0.135 M aqueous solution of periodic acid (HIO4), for which Ka = 2.3 × 10–2. Select one: A. 1.25 B. 3.28 C. 1.17 D. 1.64 E. 1.34 Question 42 Correct 4.00 points out of 4.00 In which molecule is the central atom sp2 hybridized? Select one: A. N2O B. NF3 C. SO2 D. PF5 E. BeCl2Question 46 Correct 4.00 points out of 4.00 The reaction of a strong acid with water results in Select one: A. a weak conjugate base. B. a weak conjugate acid. C. a strong conjugate base. D. a strong base. E. pure water. Question 47 Correct 4.00 points out of 4.00 Which is the correct statement? Select one: A. All protons are lost from a polyprotic acid at the same time. B. H2O is a diprotic acid. C. NH3 is a polyprotic acid. D. NH3 is a diprotic acid. E. A polyprotic acid has more than two ionizable protons. Question 45 Correct 4.00 points out of 4.00 For H3PO4, Ka1 = 7.3 × 10–3, Ka2 = 6.2 × 10–6, and Ka3 = 4.8 × 10–13. A 0.10 M aqueous solution of Na3PO4 therefore would be . Select one: A. weakly basic B. neutral C. strongly basic D. weakly acidic E. strongly acidicQuestion 49 Correct 4.00 points out of 4.00 A 0.15 M solution of chloroacetic acid has a pH of 1.86. What is the value of Ka for this acid? Select one: A. 7.2 × 101 B. 9.9 × 10–2 C. 1.6 × 10–1 D. 2.7 × 10–4 E. 1.4 × 10–3 Question 50 Correct 4.00 points out of 4.00 The substance NH3 is considered to be Select one: A. a strong base. B. a neutral compound. C. a weak acid. D. a strong acid. E. a weak base. Question 48 Correct 4.00 points out of 4.00 Which is an amphoteric oxide? Select one: A. Al2O3 B. MgO C. SO2 D. Na2O E. Cl2O7Quiz navigation Show one page at a time Finish review 1 2 3 4 5 6 7 8 9 10 26 27 38 39 40 41 42 48 49 50 © 2023 StraighterLine. All rights reserved