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Name: Click here to enter text.Basic Stoichiometry PhET LabLet's make some sandwiches!5259705170815Introduction:When we bake/cook something, we use a specific amount of each ingredient. Imagine if you made a batch of cookies and used way too many eggs, or not enough sugar. In chemistry, reactions proceed with very specific recipes. The study of these recipes is stoichiometry. When the reactants are present in the correct amounts, the reaction will produce products. What happens if there are more or less of some of the reactants present? Vocabulary:Before you begin, please define the following:Limiting Reactant:Click here to enter text.Excess Reactant: Click here to enter text.Synthesis Reaction: Click here to enter text.Combustion Reaction: Click here to enter text.Mole Ratio: Click here to enter text.Diatomic Molecule: Click here to enter text.Mole: Click here to enter text.Hydrocarbon: Click here to enter text.Procedure: PhET Simulations Play with the Sims Chemistry Reactants, Products, and LeftoversIf a yellow bar drops down in your browser, click on it and select "Allow Blocked Content"Part 1: Making Sandviches: The is a simulation of a two-reactant synthesis reaction. In this case, one reactant will be limiting, while the other will be in excess. Take some time and familiarize yourself with the simulation.Set the reaction to a simple mole ratio of 2:1:1Complete the table below while making tasty cheese sandwiches:Bread UsedCheese UsedSandwiches MadeExcess BreadExcess Cheese5 slices5 slicesClick here to enter text.Click here to enter text.Click here to enter text.4 slices3slicesClick here to enter text.Click here to enter text.Click here to enter text.Click here to enter text.Click here to enter text.2 sandwiches1 slice0 slices6 slicesClick here to enter text.3 sandwichesClick here to enter text.4 slicesPart 2: Real Chemical Reactions: 5316855-134620Now let's work with real chemical reaction, one that creates a very entertaining BOOM!What is the mole ratio for the reaction of hydrogen and oxygen to produce water? Click here to enter text.H2+ Click here to enter text. O2────────────────── Click here to enter text.H2OComplete the table below while making water H2O from hydrogen H2 and oxygen O2: Hydrogen Molecules H2Oxygen Molecules O2Water Molecules H2OExcess H2Excess O24 molecules4 moleculesClick here to enter text.Click here to enter text.Click here to enter text.7 molecules6 moleculesClick here to enter text.Click here to enter text.Click here to enter text.Click here to enter text.Click here to enter text.4 molecules0 molecules0 molecules9 moles8 molesClick here to enter text.Click here to enter text.Click here to enter text.Hydrogen Molecules H2Oxygen Molecules O2Water Molecules H2OExcess H2Excess O2Click here to enter text.Click here to enter text.4 moles1 moles0 moles4.0 moles2.5 molesClick here to enter text.Click here to enter text.Click here to enter text.1.5 molesClick here to enter text.1.5 moles0 moles0 moles5631180281305Notice that the labels changed from molecules to moles. This does not change the mole ratio, as a mole is simply a large number of molecules. How many molecules is a mole? Click here to enter text.Now try producing ammonia, a very important chemical in industry and farming.What is the mole ratio for the production of ammonia? Click here to enter text.Complete the table below:Moles N2Moles H2Moles NH3Excess N2Excess H23 moles6 molesClick here to enter text.Click here to enter text.Click here to enter text.6 moles3 molesClick here to enter text.Click here to enter text.Click here to enter text.Click here to enter text.Click here to enter text.4 moles2 moles0 moles1.5 moles4.0 molesClick here to enter text.Click here to enter text.Click here to enter text.Combustion of hydrocarbons like methane CH4 produces two products, water and carbon dioxide CO2.What is the mole ratio for the combustion of methane? Click here to enter text.Complete the table below: WATCH FOR FRACTIONSmol CH4mol O2mol CO2mol H2OExcess mol CH4Excess mol O24 mol4 molClick here to enter text.Click here to enter text.Click here to enter text.Click here to enter text.3 mol6 molClick here to enter text.Click here to enter text.Click here to enter text.Click here to enter text.Click here to enter text.Click here to enter text.2 mol4 molClick here to enter text.Click here to enter text.Click here to enter text.Click here to enter text.3 molClick here to enter text.Click here to enter text.Click here to enter text. Basic Stoichiometry Post-Lab ExercisesComplete each exercise. Remember to use proper units and labels.1.For the reaction determine the correct lowest mole ratio.Click here to enter text.2.For the reaction determine the correct lowest mole ratio.Click here to enter text.3.For the reaction, determine how many moles of chlorine Cl2 would be needed to react with 3 moles of phosphorus P4 to entirely use up all the phosphorus.4) Click here to enter text.4.If 5 moles of P4 reacted with 22 moles Cl2 according to the above reaction, determine:a) How many moles PCl3 are produceda) Click here to enter text.b) How many moles of P4 are left in excess after the reaction (if any)b) Click here to enter text.c) How many moles of Cl2 are left in excess after the reaction (if any)c) Click here to enter text.-9334514414500In reality, reactants don't have to react in perfect whole-numbers of moles. In a two-reactant synthesis reaction, usually one reactant gets entirely used up (and determines how much product is made), even if that means using fractions of a mole of reactant. For instance, when solid, metallic aluminum Al and red, liquid bromine Br2 are brought together, they make a white solid according to the reaction . If 5.0 moles of aluminum Al was reacted with 10 moles bromine Br2, all five moles of aluminum would react, with only 7.5 moles bromine. (2:3 mole ratio) This would produce only 5.0 moles of AlBr3, leaving 2.5 moles of excess Br2 behind.5.Now assume 3 moles Al and 4 moles Br2 reacta) Which chemical is the limiting reactant?a) Click here to enter text.b) Which chemical must be the excess reactant?b) Click here to enter text.c) How much (in moles) AlBr3 gets produced?c) Click here to enter text.Click to show work here.d) If all the limiting reactant gets used up, how much of the excess reactant is left? d) Click here to enter text.Click to show work here.6.What is the maximum amount (in moles) of NaCl that can be produced from 4.5 moles of Na and 3.5 moles of Cl2 according to the reaction (left for you to balance). 7) Click here to enter text.Click to show work here.
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