SOL Review Game 1

Pick A Number 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30 31 32 33 34 35 36 37 38 39 40

Question 1 Molar Mass Density Polar Melting Point (C) Boiling Point Benzene 78.11 .878 No 5.5 80 Methanol 32.04 .791 Yes -97 65 Hexane 86.18 .659 -91 98 Octane 114.23 .702 -57 126 Water 18.0 1.0 0.0 100 A student needed to dissolve a substance that she knew was soluble in water. According to the chart, which other solvent would most likely dissolve the substance?

Question 1 Return Molar Mass Density Polar Melting Point (C) Boiling Point (C) Benzene 78.11 .878 No 5.5 80 Methanol 32.04 .791 Yes -97 65 Hexane 86.18 .659 -91 98 Octane 114.23 .702 -57 126 Water 18.0 1.0 0.0 100 A student needed to dissolve a substance that she knew was soluble in water. According to the chart, which other solvent would most likely dissolve the substance? Answer: Methanol – you’re looking for the polar substance Like dissolves like!! Return

Question 2 How much energy is required to convert 15 g of chloroform from liquid to vapor? (Ch 5) a) 4.0 calories b) 59 calories c) 885 calories d) 3060 calories

Question 2 Answer How much energy is required to convert 15 g of chloroform from liquid to vapor? c) 885 calories 15 g x 59 cal/g = 885 cal Return

Question 3 One way to increase the volume of the gas in the balloon in the diagram above is to — (Ch 4-5) F cool the gas in the balloon only G increase the temperature of the water H push the balloon farther down into the water bath J seal the top of the water bath

Question 3 One way to increase the volume of the gas in the balloon in the diagram above is to — (Ch 4-5) G increase the temperature of the water Return

Question 4 H2(g) + I2(g)  2 HI(g) Ten moles of hydrogen and ten moles of iodine were put into a sealed 1-liter container at 490 C and allowed to react. After a while, there were still small amounts of unreacted hydrogen and iodine, but the hydrogen iodide concentration became constant. This is because: a) there was not enough hydrogen to react with all of the iodine b) the hydrogen iodide was reacting with the container c) iodine loses its reactivity at high temperatures d) the reaction reached a state of equilibrium

Question 4 H2(g) + I2(g) 2 HI(g) Ten moles of hydrogen and ten moles of iodine were put into a sealed 1-liter container at 490 C and allowed to react. After a while, there were still small amounts of unreacted hydrogen and iodine, but the hydrogen iodide concentration became constant. This is because: d) the reaction reached a state of equilibrium Return

Question 5 2 C2H6 + 7 O2 → 4 CO2 + 6 H2O How many moles of oxygen are required to completely react with 20 moles of ethane (C2H6)? a) 2.9 b) 40 c) 60 d) 70

Question 5 2 C2H6 + 7 O2 → 4 CO2 + 6 H2O How many moles of oxygen are required to completely react with 20 moles of ethane (C2H6)? d) 70 Return

Question 6 Sodium iodide exhibits what type of bond? a) Covalent b) Ionic c) Hydrogen d) Metallic

Question 6 Sodium iodide exhibits what type of bond? b) Ionic Return

Question 7 Which of the following reactions is a decomposition reaction? a) S8 + 8 O2 → 8 SO2 b) O2 + 2 H2O → 2 H2O2 c) 2 KClO3 → 2 KCl + 3 O2 d) Na + AgCl → NaCl + Ag

Question 7 Which of the following reactions is a decomposition reaction? c) 2 KClO3 → 2 KCl + 3 O2 Return

Question 8 Which of the following reactions is not balanced? a) S8 + 8 O2 → 8 SO2 b) O2 + H2O → H2O2 c) 2 KClO3 → 2 KCl + 3 O2 d) Na + AgCl → NaCl + Ag

Question 8 Which of the following reactions is not balanced? b) O2 + H2O → H2O2 Return

Question 9 An alkali metal will most readily react with — a) another alkali metal b) an alkaline earth metal c) a halogen d) a noble gas

Question 9 An alkali metal will most readily react with — c) a halogen Return

Question 10 Element X has three isotopes. X-100 occurs 94% of the time, X-101 occurs 4% of the time and X-102 occurs 2% of the time. What is the average atomic mass of element X? a) 101.0 amu b) 100.3 amu c) 100.1 amu d) 100.0 amu

Question 10 Element X has three isotopes. X-100 occurs 94% of the time, X-101 occurs 4% of the time and X-102 occurs 2% of the time. What is the average atomic mass of element X? c) 100.1 amu Return

Question 11 What is the percentage of nitrogen in ammonia (NH3)? b) 82% c) 80% d) 25%

Question 11 What is the percentage of nitrogen in ammonia (NH3)? b) 82% Return

Question 12 How does the isotope U -238 differ from its counterpart U -235? a) It has a different number of protons and three less neutrons than U -235. b) It has the same number of protons and three more electrons than U -235. c) It has the same number of protons but three more neutrons than U -235. d) It has a different number of protons and three more neutrons than U -235.

Question 12 How does the isotope U -238 differ from its counterpart U -235? c) It has the same number of protons but three more neutrons than U -235. Return

Question 13 Magnesium forms a +2 ion. How many electrons does a magnesium ion have? a) 14 b) 12 c) 10 d) 2

Question 13 Magnesium forms a +2 ion. How many electrons does a magnesium ion have? a) 14 b) 12 c) 10 d) 2 Return

Question 14 An element has an electron configuration of 1s22s22p63s1. Which of these will be in the same group as this element? a) 1s22s22p6 b) 1s22s22p63s23p64s1 c) 1s22s22p63s2 d) 1s22s22p63s23p6

Question 14 An element has an electron configuration of 1s22s22p63s1. Which of these will be in the same group as this element? b) 1s22s22p63s23p64s1 Return

Question 15 Electronegativity differences are often helpful in determining the bond character between two atoms. A general rule states that if the electronegativity difference between two atoms is greater than 1.67, an ionic bond would most likely be formed. Using the chart above, which pair of atoms would probably form the strongest ionic bond? A N-O B Na-F C K-Cl D Mg-O

Question 15 Electronegativity differences are often helpful in determining the bond character between two atoms. A general rule states that if the electronegativity difference between two atoms is greater than 1.67, an ionic bond would most likely be formed. Using the chart above, which pair of atoms would probably form the strongest ionic bond? B Na-F Return

Question 16 Which of the following scientists performed the above experiment? a) Thomson b) Millikan c) Bohr d) Rutherford

Question 16 Which of the following scientists performed the above experiment? d) Rutherford Return

Question 17 Which is the correct formula for iron (II) sulfate? a) Fe3(SO4)2 b) FeSO4 c) Fe2(SO4)3 d) Fe2(SO3)3

Question 17 Which is the correct formula for iron (II) sulfate? b) FeSO4 Return

Question 18 Which of these elements is found in a group with the electron configuration ns2np1? a) Be b) Al c) Ge d) Sb

Question 18 Which of these elements is found in a group with the electron configuration ns2np1? b) Al Return

Question 19 The pH of a 0.001 molar aqueous solution of HCl would equal — a) -3 b) 1 c) 3 d) 11

Question 19 The pH of a 0.001 molar aqueous solution of HCl would equal — c) 3 Return

Question 20 The system that shows a decrease in entropy (disorder) is — a) sublimation of CO2 b) ice melting c) combustion of gasoline d) water freezing

Question 20 The system that shows a decrease in entropy (disorder) is — d) water freezing Return

Question 21 The scientist who used the above experimental setup to discover the electron is – a) Rutherford b) Heisenberg c) Bohr d) Thomson

Question 21 The scientist who used the above experimental setup to discover the electron is – d) Thomson Return

Question 22 What is the density of N2 gas at STP? a) 1.60 g/mL b) 1.25 g/mL c) 0.80 g/mL d) 0.63 g/mL

Question 22 What is the density of N2 gas at STP? b) 1.25 g/mL Return

Question 23 Which of these is about 2 moles? a) 2.0 liters of H2 b) 4.0 grams of H2 c)2.0 x 1023 molecules of H2 d)4.0 kilograms of H2

Question 23 Which of these is about 2 moles? b) 4.0 grams of H2 Return

Question 24 During combustion, methane yields carbon dioxide and water. The unbalanced equation for this reaction is: CH4(g) + O2(g) CO2(g) + H2O(l) What will be the coefficients for the balanced equation be? (What coefficients are needed in order to balance this equation?)   A. 1 : 1 : 2 : 1 B. 5 : 4 : 3 : 6 C. 1 : 1 : 1 : 2 D. 1 : 2 : 1 : 2

Question 24 During combustion, methane yields carbon dioxide and water. The unbalanced equation for this reaction is: CH4(g) + O2(g) CO2(g) + H2O(l) What will be the coefficients for the balanced equation be? (What coefficients are needed in order to balance this equation?)   D. 1 : 2 : 1 : 2 Return

Question 25 Consider the following balanced reaction: 4NH3 (g) + 5O2 (g) 4NO (g) + 6H2O (g) How many grams of ammonia are required to react completely with 40 g of oxygen?   A. 19 g B. 15 g C. 17 g D. 34 g

Question 25 Consider the following balanced reaction: 4NH3 (g) + 5O2 (g) 4NO (g) + 6H2O (g) How many grams of ammonia are required to react completely with 40 g of oxygen?   C. 17 g Return

Question 26   What is the molecular formula for a compound with a molar mass of 26 g/mol and an empirical formula of CH? A. CH B. C2H C. C2H2 D. C3H3

Question 26 What is the molecular formula for a compound with a molar mass of 26 g/mol and an empirical formula of CH?   C. C2H2 Return

Question 27 What volume of a 0.50 M MgSO4 solution will be needed to prepare 100.0 mL of a 0.20 M MgSO4 solution?   A. 100 mL B. 0.250 mL C. 40.0 mL D. 250 mL

Question 27 What volume of a 0.50 M MgSO4 solution will be needed to prepare 100.0 mL of a 0.20 M MgSO4 solution?   C. 40.0 mL Return

Question 28 Nitrous oxide (N2O), or laughing gas, is commonly used as an anesthetic in dentistry and surgery. How many moles are present in 8.4 liters of nitrous oxide at STP?   A. 25.2 moles B. 0.375 moles C. 0.19 moles D. 5.2 moles

Question 28 Nitrous oxide (N2O), or laughing gas, is commonly used as an anesthetic in dentistry and surgery. How many moles are present in 8.4 liters of nitrous oxide at STP?   B. 0.375 moles Return

Question 29 Calculate the approximate number of molecules in a drop of water with a mass of 0.10 g.   A. 4 x 1023 molecules B. 6 x 1021 molecules C. 3 x 1021 molecules D. 2 x 1023 molecules

Question 29 Calculate the approximate number of molecules in a drop of water with a mass of 0.10 g.   C. 3 x 1021 molecules Return

Question 30 Which of the following statements is correct according to the Bronsted-Lowry definition of an acid?   A. Acids release a hydrogen ion and are proton donors. B. Acids release a hydrogen ion and are proton acceptors. C. Acids release a hydroxide ion and are proton acceptors. D. Acids release a hydroxide ion and are proton donors.

Question 30 Which of the following statements is correct according to the Bronsted-Lowry definition of an acid?   A. Acids release a hydrogen ion and are proton donors. Return

Question 31 Which of the following statements best describes what determines whether an acid is a strong acid or a weak acid?   A. the number of hydrogen ions in the molecule B. the amount of solvent in which it is dissolved C. the degree to which it dissociates in water D. the extent to which it reacts with the solvent

Question 31 Which of the following statements best describes what determines whether an acid is a strong acid or a weak acid?   C. the degree to which it dissociates in water Return

Question 32 In human cells, a dynamic equilibrium exists between carbonic acid and carbon dioxide. H2CO3 (aq)     CO2 (g) + H2O (l) When a person exercises, however, the body's cells metabolize glucose to gain energy, but this metabolism also causes an increase in the concentration of carbon dioxide. According to Le Chatelier's Principle, how does this affect the system?   A. There is a decrease in the concentration of carbonic acid. B. There is a decrease in the concentration of water. C. There is an increase in the concentration of glucose. D. There is an increase in the concentration of carbonic acid.

Question 32 In human cells, a dynamic equilibrium exists between carbonic acid and carbon dioxide. H2CO3 (aq)     CO2 (g) + H2O (l) When a person exercises, however, the body's cells metabolize glucose to gain energy, but this metabolism also causes an increase in the concentration of carbon dioxide. According to Le Chatelier's Principle, how does this affect the system?   D. There is an increase in the concentration of carbonic acid. Return

Question 33 Consider the following reaction: energy + 2 HgO (s)     2 Hg (l) + O2 (g) This reaction is   A. an exothermic reaction. B. a synthesis reaction. C. a single-replacement reaction. D. an endothermic reaction.

Question 33 Consider the following reaction: energy + 2 HgO (s)     2 Hg (l) + O2 (g) This reaction is   D. an endothermic reaction. Return

Question 34 Which of the following sets of coefficients correctly balances the following chemical equation?      Al(OH)3          Al2O3 +      H2O   A. 2; 2; 3 B. 3; 1; 2 C. 2; 1; 2 D. 2; 1; 3

Question 34 Which of the following sets of coefficients correctly balances the following chemical equation?      Al(OH)3          Al2O3 +      H2O   D. 2; 1; 3 Return

Question 35 A 20-liter cylinder contains 4 moles of natural gas. The temperature of the cylinder is 274 K. Assuming that the gas is ideal and using the universal gas constant of 0.08206 L-atm/mol-K, what is the approximate pressure in the cylinder?   A. 4.5 atm B. 22.5 atm C. 54.8 atm D. 112.4 atm

Question 35 A 20-liter cylinder contains 4 moles of natural gas. The temperature of the cylinder is 274 K. Assuming that the gas is ideal and using the universal gas constant of 0.08206 L-atm/mol-K, what is the approximate pressure in the cylinder?   A. 4.5 atm Return

Question 36 Which statement below describes Charles’ law?   A. Volume is inversely proportional to temperature. B. Pressure is inversely proportional to temperature. C. Volume is proportional to temperature. D. Pressure is proportional to temperature.

Question 36 Which statement below describes Charles’ law?   C. Volume is proportional to temperature. Return

Question 37 Free Point 

Question 37 Free Point  Return

Question 38 How much heat is absorbed when 75 g of liquid carbon tetrachloride (CCl4) vaporizes into a gas? (The heat of vaporization of CCl4 is 53.8 cal/g.)   A. 1.394 calories B. 4035 calories C. 0.717 calories D. 128.8 calories

Question 38 How much heat is absorbed when 75 g of liquid carbon tetrachloride (CCl4) vaporizes into a gas? (The heat of vaporization of CCl4 is 53.8 cal/g.)   B. 4035 calories Return

Question 39 The temperature of 100 g of water rises from 25°C to 30°C when an acid is reacted with a base in a calorimeter. Calculate the enthalpy change (ΔH) for the reaction. The specific heat of water is 4.18 J g-1°C-1.   A. 3000 J B. 2090 J C. 717.7 J D. 119.6 J

Question 39 The temperature of 100 g of water rises from 25°C to 30°C when an acid is reacted with a base in a calorimeter. Calculate the enthalpy change (ΔH) for the reaction. The specific heat of water is 4.18 J g-1°C-1.   B. 2090 J Return

Question 40 Which of the below values of temperature and pressure will yield a sample of dry ice? A. 0°C and 70 atm B. -80°C and 1 atm C. 32°C and any pressure D. 31.1°C and 2 atm

Question 40 Which of the below values of temperature and pressure will yield a sample of dry ice? B. -80°C and 1 atm Return