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Exam 1 ReviewSupplemental InstructionIowa State UniversityLeader:KiaCourse:CHEM 177Instructor:KingstonDate:February 3rd, 2017Determine whether the following is a physical or chemical processRusting metal canBoiling a cup of waterPulverizing (crushing) aspirinDigesting a candy barExploding nitroglycerin Label the following groups on the periodic tableChalcogensHalogensAlkali metalsNoble gasesAlkaline earth metalsMetalloids Give examples of the followingIntensive propertyExtensive propertyHeterogeneous mixtureHomogeneous mixturePure substanceFill in the following table with the appropriate charges (for more polyatomic ions see slides from lecture 6)Element/polyatomic compoundChargeElement/polyatomic compoundChargeKOH (hydroxide ion)ClNAlZnNH4 (ammonium ion)NO3 (nitrate ion)Name the all of the diatomic elementsCalculate the followingWhat is the mass, in grams, of 2.50 x 10-3 mol of ammonium phosphate ((NH4)3PO4)?How many moles of chloride ions are in 0.2550 g of aluminum chloride? What is the mass, in grams, of 7.70 x 1020 molecules of caffeine, C8H10N4O2?What is the molar mass of cholesterol if 0.00105 mol has a mass of 0.406 g?Fill in the following tableSymbol112CdProtons3892Neutrons5849Electrons3836Mass no.81235Solve the following dimensional analysis questionsAn individual suffering from a high cholesterol level in her blood has 242 mg of cholesterol per 100 mL of blood. If the total blood volume of the individual is 5.2 L, how many grams of total blood cholesterol does the individual’s body contain? In March 1989 the Exxon Valdez ran aground and spilled 240,000 barrels of crude petroleum off the coast of Alaska. One barrel of petroleum is equal to 42 gal. How many liters of petroleum were spilled? (1 gal = 3.79 L)Automobile batteries contain sulfuric acid, which is commonly referred to as “battery acid.” Calculate the number of grams of sulfuric acid in 1.00 gal of battery acid if the solution has a density of 1.28 g/mL and is 38.1% sulfuric acid by mass.Find the empirical and molecular formula of Styrene given the following percent compositions and a molar mass of 104 g/mol. You can use the following table to help with calculations Percent composition g in 100 g sampleMolar massmolesMole ratiosCarbon92.3 %Hydrogen 7.7 % Hydrogen sulfide is an impurity in natural gas that must be removed. One common removal method is called the Claus process, which relies on the reaction (balance the equation yourself!): __ H2S(g) + __ O2(g) __ S8(l) + __ H2O(g)Under optimal conditions the Claus process gives 98% yield of S8 from H2S. If you started with 30.0 grams of H2S and 50.0 grams of O2, how many grams of S8 would be produced, assuming 98% yield? CHALLENGE PROBLEMSA compound whose empirical formula is XF3 consists of 65% F by mass. What is the atomic mass of X? Rubidium has two naturally occurring isotopes, 85Rb (relative mass 84.9118 amu) and 87Rb (relative mass 86.9092 amu). If rubidium has an average atomic mass of 85.47 amu, what is the abundance of each isotope (in percent)?I have 3 moosigles of apples. I know that 1 moosigle is approximately the weight of 42.6 squirrels and 3.7 squirrels weigh the same as an average sized dog. Given that the average weight of a dog is 26 gaggles, what is the weight of my apples in gaggles?The length and width of a box, respectively, 18 cm and 15 cm. If the box holds 6.0 kg of water, what is the height of the box? (water density = 1.0 g/ml)Gold can be hammered into extremely thin sheets called gold leaf. An architect wants to cover a 100 ft x 82 ft ceiling with gold leaf that is five-millionths of an inch thick. The density of gold is 19.32 g/cm^3, gold costs $1654 per troy ounce (1 tory ounce = 31.1034768 g). How much will it cost the architect to buy the necessary gold? Extra PracticeBalance and determine the type of the following reactions.__Fe(s) + __O2(g) → __Fe2O3(s)__KCl(s) → __K(s) + __Cl2(g)__C8H18(g) + __O2(g) → __CO2(g) + __H2O(l)Which of the following lengths is the largest?6.7 m8.9 x 10-6 km7.3 x 1010 nm5.4 x 103 mmCircle the lowest temperature, underline the highest temperature *careful!*72 ℉22.2 ℃290 K Convert the atomic mass of one molecule of water into pounds ................
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