1 Explain why salt water is a homogenous mixture 2 Convert 78 F to Kelvin 3 A piece of metal has a mass of 12 3 grams and displaces 1 3 mL of water a Calculate the density of the metal in g mL b Convert this density to kg m3 4 What is the percent composition of a Carbon in carbon dioxide b Hydrogen in water c Sulfur in sulfuric acid 5 Name the following a NaCl b PCl5 c NH4 3PO3 d HClO4 6 A substance containing only carbon hydrogen and oxygen is burned to produce 9 64 grams of carbon dioxide and 3 94 grams of water The total mass of compound was 6 57 grams a How much carbon was in the compound b How much hydrogen was in the compound c How much oxygen was in the compound d What is the empirical formula of the compound e If the molar mass of the compound is 180 g mol what is the molecular formula of the compound 7 Consider a new element element X Element X has 2 known isotopes 353X and 355X If the percent composition for each isotope is 37 3 and 62 3 respectively what is the average atomic mass of element X 8 78 9 grams of propane is mixed with an equal mass of oxygen a Write a balanced chemical equation that describes this scenario b Which reactant is the limiting reagent c If only 49 7 grams of carbon dioxide are collected what is the percent yield of the reaction 9 Convert 9 23x1027 molecules of ammonia to grams 10 Write balanced net ionic equations for the following a Solutions of silver acetate and sodium chloride are mixed i Identify the precipitate b Solutions of hydrochloric acid and potassium hydroxide are mixed i What is the pH of the resultant solution c Zinc metal is placed in a solution of sulfuric acid i What is the name of the gas produced d Zinc metal is placed in a solution of copper sulfate i What is one major obvious indication of this reaction 11 Hydrogen peroxide breaks down to form water and oxygen gas a Which element is reduced b Which element is oxidized 12 Identify the following as a strong electrolyte weak electrolyte or nonelectrolyte a Propane b Acetic acid c Lithium chloride 13 The volume of the gas inside a light bulb is about 350 mL When the light is off and the temperature of the gas inside the bulb is 25 C the pressure inside the bulb is 1 01 atm a What is the pressure inside the light bulb when it s been left on for 6 hours and reaches a temperature of 73 C b Convert this pressure to mmHg 14 What mass of ethane C2H6 occupies a balloon with a volume of 96 5 centiliters cL at a temperature of 35 C and a pressure of 765 Torr 15 A certain gas has a density of 1 81 g L at a temperature of 25 C and a pressure of 1 01 atmospheres A second gas methane CH4 effuses at a rate of 23 L min a What is the rate of effusion for the unknown gas 16 5 6 grams of zinc is placed in 250 mL of 2 5 M hydrochloric acid The reaction takes place at STP a What volume of gas is produced b Calculate the work done by this gas in Joules c If the reaction releases 350 J of energy what is the change in internal energy 17 33 5 grams of iron specific heat 0 444 J gC is placed on top a 55 1 gram bar of gold heat capacity 0 126 J gC The initial temperature of the iron bar is 53 C and the initial temperature of the gold bar is 23 C a Calculate the temperature of each bar when they come to thermal equilibrium 18 Using standard enthalpies of formation calculate the enthalpy of reaction for the combustion of propane 19 What is the De Broglie wavelength of a 125 kg baseball traveling at a velocity of 44 3m s 20 The work function of calcium metal is 4 65x10 19 J velocity of 8 99x107 m s b What is the wavelength of this radiation a What energy must a light have in order to dislodge an electron from the metal at a 21 A volume of 250 mL of water is heated using a hydrogen lamp The specific heat of water is 4 184 J gC a How much energy is required to heat this amount of water from 25 C to 37 C b If the hydrogen lamp produces photons with a wavelength of 425 nanometers how many photons are required c Calculate the change in energy when atoms in the lamp transition from the excited state at n 5 to the ground state at n 2 22 Calculate the lattice energy of magnesium oxide using a Born Haber cycle 23 Consider the element Bromine a Write out its full electron configuration b Draw its orbital diagram c What are the quantum numbers for the 26th electron 24 Explain the following using your knowledge of periodic trends and atomic principles a The atomic radius of potassium is greater than the atomic radius of lithium b The atomic radius of chlorine is smaller than the atomic radius of sodium c The first ionization energy of chlorine is greater than the first ionization energy of phosphorus beryllium d The first ionization energy of boron is less than the first ionization energy of e The electronegativity of nitrogen is less than that of oxygen f The electron affinity of nitrogen is positive whereas the electron affinity of fluorine is negative 25 Draw the Lewis Structure s for the following a Boron trifluoride b Phosphorus dioxide i Is this molecule polar or nonpolar i What is the hybridization of the central atom c Sulfur trioxide i What is the formal charge of each atom when formal charge is minimized 26 Calculate the enthalpy of reaction for the combustion of propane using bond enthalpies 27 What is the angle between the bonds in the ammonium ion 28 Determine the molecular geometry and hybridization of the central atom in the following molecules a ICl3 b CH4 c PH5 29 How many sigma and pi bonds are found in 2 butynoic acid CH3 C C COOH 30 Explain why methane is nonpolar and ammonia is polar
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