99 Created by Master Student Chemistry Practice Test #9 1 / 30 If 49 grams of H2SO4 react with 80.0 grams of NaOH, how much reactant will be left over after the reaction is complete? 24.5 g H2SO4 none of either compound 20. g NaOH 40. g NaOH 60. g NaOH (D) H2SO4 + 2NaOH <=> 2H2O + Na2SO4 is the equation for this reaction. 1 mol H2SO4 = 98 g. 1 mol NaOH = 40 g. Then 49 g of H2SO4 = mol H2SO4. The equation shows that 1 mol of H2SO4 reacts with 2 mol of NaOH for a ratio of 1 : 2. Therefore, mol of H2SO4 reacts with 1 mol of NaOH in this reaction. Since 1 mol of NaOH equals 40. g, and 80. g of NaOH is given, 40. g of it will remain after the reaction has gone to completion. 2 / 30 A saturated solution of BaSO4 at 25 degrees C contains 3.9e 10-5 mole/liter of Ba2+ ions. What is the Ksp of this salt? 3.9e 10-5 3.9e 10-6 2.1e 10-7 1.5e 10-8 1.5e 10-9 (E) Ksp = [Ba2+] [SO42-] since [Ba2+] is given as [3.9e 10-5], and the equation BaSO4 <=> Ba2+ + SO42- shows there will be as many SO42- ions as Ba2+ ions, then both [Ba2+] and [SO42- will equal 3.9e 10-5. So, Ksp = [3.9e 10-5][3.9e 10-5] Ksp = 1.5e 10-9 3 / 30 Will be colored blue A 0.01-molar solution of HNO3 A 0.01-molar solution of HC2H3O2 A 0.01-molar solution of Cu(NO3)2 A 0.01-molar solution of NaNO3 A 0.01-molar solution of NaOH The solution containing Cu2+ ion will be blue. Most solutions containing salts of transition metals are distinctly colored because the d subshell electrons of transition metals absorb and emit electromagnetic radiation in the visible spectrum. 4 / 30 May be used in combination with a calorimeter to compare the specific heats of two substances Thermometer Conductivity tester Salt bridge Buret Graduated cylinder When we talk about specific heat, we're talking about the amount of heat necessary to produce a change in temperature. The calorimeter can be used to measure heat input or output, and the thermometer, choice (A), would be used in combination with it to ascertain the associated change in temperature. 5 / 30 The property of matter that is independent of its surrounding conditions and position is volume density mass weight state (C) Mass is a constant and is not dependent on position or surrounding conditions. 6 / 30 The forces of attraction that exist between nonpolar molecules are called Van der Waals / dispersion forces ionic bonds covalent bonds electrovalent bonds metallic bonds 0 7 / 30 Deoxyribose in DNA nucleotides belongs to this family of biologically important molecules Nucleic acids Proteins Carbohydrates Lipids Electrolytes Deoxyribose is a ribose sugar molecule missing an oxygen atom. As with all molecules with the suffix -ose, ribose is a carbohydrate. In general, proteins tend to have the suffix -in (or -ase if they are an enzyme) and nucleic acids have the suffix -ine (except for uracil). 8 / 30 The expression that can be used to designate a maximum of 3 moles of ions H2(g) CO2(g) 2N2O(g) 2NaCl (aq) H2SO4(dilute aq) (E) With complete ionization , or 3 mol of ions per mole of H2SO4. 9 / 30 Has mass and a definite size and shape Density A solid Volume Weight Matter (B) Matter that has mass and a definite size and shape is called a solid. 10 / 30 What is the approximate percentage composition by mass of the element oxygen in the compound HClO4? 16% 32% 50% 64% 75% Add up the mass of 1 mole of this substance. From the periodic table, we know that 11 / 30 Based on the solubility products given below, which of the following salts is the most soluble? BaCO3 Ksp = 5.1e 10-9 PbCrO4 Ksp = 2.8e 10-13 AgCl Ksp = 1.8e 10-10 CaSO4 Ksp = 9.1e 10-6 ZnC2O4 Ksp = 2.7e 10-8 The solubility product (Ksp) of a molecule is a measure of the concentrations of the particles into which it dissociates in solution at equilibrium. Since all of these salts will ionize into two ions per unit, the salt with the largest value of Ksp will be the most soluble. 12 / 30 Each of the following systems is at equilibrium in a closed container. A decrease in the total volume of each container will increase the number of moles of product(s) for which system? 2NH3(g) N2(g) + 3H2(g) H2(g) + Cl2(g) 2HCl(g) 2NO(g) + O2(g) 2NO2(g) CO(g) + H2O(g) CO2(g) + H2(g) Fe3O4(s) + 4H2(g) 3Fe(s) + 4H2O(g) (C) A decrease in volume will cause the equilibrium to shift in the direction that has less volume(s) of gas(es). In every case except (C) this is the reverse reaction, which decreases the product. The coefficients give the volume relationships. 13 / 30 Consist of atoms that have valence electrons in a d subshell Alkali metals Alkaline earth metals Noble gases Halogens Transition metals When the test writers start talking about the "d" subshell, think "transition metals." 14 / 30 The ratio of the rate of movement of hydrogen gas compared with the rate of oxygen gas is 4 : 1. Law of Definite Composition Nuclear fusion van der Waals forces Graham's Law of Diffusion (Effusion) Triple point (D) According to Graham's Law of Gaseous Diffusion (or Effusion), the rate of diffusion is inversely proportional to the square root of the mole cular weight. 15 / 30 Defined as a measure of the mass times the gravitational force Density A solid Volume Weight Matter (D) Weight is the product of mass times a gravitational force. In outer space where there is no gravitational force, we say a mass is weightless. 16 / 30 The joining of many hydrogen nuclei in the nuclear reaction that occurs in stars is called a mass defect sunburn fusion reaction fission reaction helium reaction 0 17 / 30 When most fuels burn, the products include carbon dioxide and hydrocarbons hydrogen water hydroxide hydrogen peroxide (C) Water is formed because most common fuels contain hydrogen in their structures. 18 / 30 Which equation is correctly balanced? Na + Cl2 <=> 2NaCl CH4 + 3O2 <=> CO2 + H2O 2KI + Pb(NO3)2 <=> 2KNO3 + PbI2 H2SO4 + KOH <=> K2SO4 + H2O C6H12O6 + 6O2 <=> 6CO2 + H2O 0 19 / 30 A product formed from a base reacting with H2SO4 Radioactive isotope Monoclinic crystal Sulfur trioxide Sulfate salt Allotropic form (E) Sulfuric acid reacts with a base to form a sulfate salt. 20 / 30 Which compound contains no ionic character? NH4Cl CaO K2O Li2O CO 0 21 / 30 If the molar concentration of Ag+ ions in 1 liter of a saturated water solution of silver chloride is 1.38e 10-5 mole/liter, what is the Ksp of this solution? 0.34e 10-10 0.69e 10-5 1.90e 10-10 2.76e 10-5 2.76e 10-10 (C) Ksp = [Ag+][Cl-] = 1.9e 10-10. The molar concentrations of Ag+ and Cl- are 1.38e 10-5 mol/L, so [Ag+][Cl-] = Ksp [1.38e 10-5][1.38e 10-5] = 1.90e 10-10 22 / 30 Holds a sample of barium iodide, BaI2, together Hydrogen bonding Ionic bonding Metallic bonding Nonpolar covalent bonding Polar covalent bonding BaI2 is composed of a metal (Ba) and nonmetal (I) bonded together. This is an ionic compound that held together by-surprise-ionic bonding. 23 / 30 When 190 grams of MgCl2 are dissolved in water and the resulting solution is 500 milliliters in volume, what is the molar concentration of MgCl2 in the solution? 2.0 M 4.0 M 8.0 M 12.0 M 16.0 M Molarity refers to moles of solute per liter of solution. We know we have 500 milliliters of solution, but we don't know how many moles of solute we have. Let's first figure out the mass of 1 mole of MgCl2. Looking at the periodic table, we find that 1 mole of Mg has a mass of 24.3 g. Two moles of Cl have a mass of about 71 g. One mole of MgCl2, therefore, has a mass of 95.3 g. 24 / 30 Element X forms the compounds XCl3 and X2O3. Element X would most likely belong to the group called alkali metals alkaline earth metals group 13 halogens noble gases 0 25 / 30 In which of the following liquids are the Van der Waals forces of attraction between the molecules weakest? Xe Kr Ar Ne He 0 26 / 30 The element that first shows some visible metallic properties at room temperature Fluorine Chlorine Bromine Iodine Astatine (D) Some physical characteristics of metal are found in iodine, the fourth halogen down in the group. 27 / 30 The expression that can be used to designate 6 moles of atoms H2(g) CO2(g) 2N2O(g) 2NaCl (aq) H2SO4(dilute aq) (C) The expression 2N2O represents two triatomic molecules or 6 mol of atoms. 28 / 30 Which kinds of bonding can be found in a sample of H2O(l)? Hydrogen bonds only Nonpolar covalent bonds only Ionic and nonpolar hydrogen bonds Both polar covalent and hydrogen bonds Metallic and ionic bonds 0 29 / 30 Five hundred milliliters of solution of 0.1 M NaBr has how many milligrams of bromine? 200 mg 400 mg 2,000 mg 4,000 mg 20,000 mg First, find the number of moles of Br?. 30 / 30 A book is lifted off of the floor and placed on a table that is one meter above the floor. The book has gained sound energy lost chemical energy gained potential energy gained kinetic energy lost nuclear energy 0 Your score is The average score is 56% LinkedIn Facebook Twitter VKontakte 0% Restart quiz Previous Quiz Next Quiz
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