3Practice45.3 g of carbon is how many moles?5.00 liters of carbon dioxide at STP is how many moles?How many molecules of hydrogen are there in 40.0 L of hydrogen gas at STP?
4Arithmetic of Equations Stoichiometry – calculation of quantities in chemical reactionsA chemical reaction tells us a few things: (recipe)N2 + 3H2 → 2NH3We can compare number of atoms, number of molecules, moles, mass and volumeWhich of these are conserved? (same on both side)
5How to interpret a reaction Given the reaction: N2 + 3H2 → 2NH3We can easily get number of each atom, each molecule, and volume of each gas.The tricky one is the mass of the reactants and products.By the law of conservation of mass, we know that each side of an equation needs to have an equal mass, but we need to find the mass of each side to show that they are equal.
6Mass of Reactants and Products N2 + 3H2 → 2NH3Reactants: 1 mol N2 = 28 g3 mol H2 = 3 X 2 g = 6 gTotal = 34 gProducts: 2 mol NH3 = 2 X 17 g = 34 gBoth sides are 34 g, which is a good sign the calculation was done right
7Now try this out Given the reaction 2Mg + O2 → 2MgO Find the number of moles and mass of reactants and productsNext do the same for this unbalanced reactionThat means YOU need to balance it!H2SO4 + NaOH → Na2SO4 + H2O
8Mole RatiosMole ratio: conversion factor derived from the coefficients of a balanced chemical reactions in terms of molesN2 + 3H2 → 2NH3This equation gives us three mole ratiosNitrogen to hydrogen, nitrogen to ammonia, and hydrogen to ammonia or1 mol N2 1 mol N2 3 mol H23 mol H2 2 mol NH3 2 mol NH3
9Get all mole ratios for this reaction 2Mg + O2 → 2MgO
10Using mole ratiosWe can use mole ratios to convert from moles of one substance to moles of a different one.If we have 3.50 mol N2 and excess H2 in the reaction: N2 + 3H2 → 2NH3How many moles of NH3 will be formed?What if we had 3.50 mol H2 and excess N2?
11Now you try these Given the equation: 2Mg + O2 → 2MgO How many moles of oxygen will react with 5.00 mol Mg?How many moles of Mg and O2 reacted if we ended up with 3.70 mol MgO?
12Mass-Mass Calculations With our new tool, the mole ratio, we can calculate the mass of any other substance in a reaction if we are given the mass of one.It will take THREE steps:Convert given grams to given moles (molar mass)Convert given moles to wanted moles(Mole Ratio)Convert wanted moles to wanted grams (molar mass)
13Example Given the reaction: N2 + 3H2 → 2NH3 How many grams of ammonia will be formed if 50 g of nitrogen react?Given the same amount of nitrogen, how much hydrogen reacted?
14Your turn Given the reaction: 2Mg + O2 → 2MgO How many grams of Mg reacted if 75.3 g MgO were formed?How many grams of O2 reacted if 75.3 g MgO were formed?
15Other Stoichiometric Calculations Instead of doing a mass-mole conversion, we can do the two other conversions from Ch 10.Instead of giving a mass, we could get a volume or number of particlesAlso, instead of calculating mass at the end, we can get volume or number of particlesLook at Figure 12.8 on page 363
16Modified Steps Convert given grams, liters or particles to given moles Convert given moles to wanted moles(Mole Ratio)Convert wanted moles to wanted grams, liters or particles
17Examples Given the reaction: 2Mg + O2 → 2MgO How many atoms of Mg reacted if 75.3 g MgO were formed?Given the reaction: N2 + 3H2 → 2NH3How many liters of ammonia will be formed if 3.50 L of nitrogen react?
18Limiting Reagent and Percent Yield Limiting reagent is the more practical application of stoichiometry that can be used in the laboratoryPercent yield compares the amount of product formed in an experiment compared to what the maximum would be
19Limiting and Excess Reactants Limiting Reactant- reactant that is used up in a reaction, which limits that amount of productExcess Reactant- reactant that remains after the reaction has stopped
20Determining a limiting reactant For these problems, we will be given the starting amounts of two reactantsWe need to use both and use each to get the amount of one of the products formed
21N2 + 3H2 → 2NH3If 5.3 moles of nitrogen gas react with 5.3 moles of hydrogen gas, how many moles of ammonia is produced? Which reactant is limiting?
22N2 + 3H2 → 2NH3If 30.0 g of nitrogen gas react with 30.0 g of hydrogen gas, how many grams of ammonia is produced? Which reactant is limiting?
23Your turn2Mg + O2 → 2MgOWhich reactant is limiting if 20.0 g of magnesium react with 20.0 g of oxygen? How much product will be formed?
24Yield DefinitionsTheoretical Yield- maximum amount of product that can be formed by the given amount of reactantsActual Yield- amount of product actually formed when an experiment is performedPercent Yield- ratio of the actual yield to the theoretical yield expressed as a percent
25Percent Yield Tells us how efficient an experiment was Can be as a result of an error made or may just be a result of the procedure of the experimentActual yield is determined in the laboratory or given in the problemTheoretical yield is determined with a calculation
26ExampleN2 + 3H2 → 2NH3If 10.0 g nitrogen react with 3.00 g hydrogen and 10.0 g ammonia is formed, what is the percent yield?
27Practice2Mg + O2 → 2MgOIf 15.0 g magnesium react with 10.0 g oxygen to form 16.5 g magnesium oxide, what is the percent yield?