Lecture 8 post

Lecture 8 post - Chapter 4 Chemical Quantities and Aqueous...

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Unformatted text preview: Chapter 4 Chemical Quantities and Aqueous Reactions Methanol burns in air according to the equation 2CH 3 OH + 3O 2 2CO 2 + 4H 2 O How many moles of O 2 are required to completely consume 2 moles of CH 3 OH ? How many moles of O 2 are required to completely consume 4 moles of CH 3 OH ? If 2 moles of CH 3 OH are burned, how many moles of H 2 O will be produced? If 6 moles of CH 3 OH are burned, how many moles of H 2 O will be produced? Numerical Relationships in a Chemical Equation ( Stoichiometry ) Estimate the mass of CO 2 produced in 2004 by the combustion of 3.4 x 10 15 g gasoline • assuming that gasoline is octane, C 8 H 18 , the reaction is: 2 C 8 H 18 ( l ) + 25 O 2 ( g ) → 16 CO 2 ( g ) + 18 H 2 O( g ) • the equation gives the mole relationship between C 8 H 18 and CO 2 , but we need the mass relationship, so g C 8 H 18 mol CO 2 g CO 2 mol C 8 H 18 Practice According to the following equation, how many milliliters of water are made in the combustion of 9.0 g of glucose? C 6 H 12 O 6 ( s ) + 6 O 2 ( g ) → 6 CO 2 ( g ) + 6 H 2 O ( l ) Limiting Reactant • for reactions with multiple reactants, it is likely that one of the reactants will be completely used before the others when this reactant is used up, the reaction stops and no more product is made • the reactant that limits the amount of product is called the limiting reactant/reagent the limiting reactant gets completely consumed • reactants not completely consumed are called excess reactants • the amount of product that can be made from the limiting reactant is called the theoretical yield • THE MOLES OF PRODUCT ARE ALWAYS DETERMINED BY THE STARTING MOLES OF LIMITING REACTANT! Things Don’t Always Go as Planned!Things Don’t Always Go as Planned!...
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This note was uploaded on 05/20/2008 for the course CHEM 115 taught by Professor Larkin during the Spring '08 term at Bloomsburg.

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Lecture 8 post - Chapter 4 Chemical Quantities and Aqueous...

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