smartbook 4

correctly order the steps necessary to calculate the mass of product formed in a chemical reaction, given the masses of all reactants.

-determine the moles of each reactant present by dividing its mass by its molar mass -determine the amount of product that could be formed from each reactant using the appropriate mole ratios -identify the limiting reactant as the reactant that produces the least amount of product -to find the mass, multiply the number of moles of product formed (from the limiting reactant) by the molar mass of the product

what is the percent yield formula?

actual yield / theoretical yield x 100

which of the following statements correctly describes the information conveyed by the balanced equation : 16Cu(s) + S8(g) --> 8Cu2S(s) -16 grams of Cu react with 1 gram of S8 to form 8 grams of Cu2S -Cu and S8 are reactants and Cu2S is the product -16 atoms of Cu react with 1 molecule of S8 to form 8 formula units of Cu2S -16 moles of Cu react with 1 mole of S8 to form 8 moles of Cu2S

-Cu and S8 are reactants and Cu2S is the product -16 atoms of Cu react with 1 molecule of S8 to form 8 formula units of Cu2S -16 moles of Cu react with 1 mole of S8 to form 8 moles of Cu2S

which of the following statements correctly interpret the balanced chemical equation : 4HCl(aq) + MnO2(s) --> MnCl2(aq) + 2H2O(g) + Cl2(g)? select all that apply -liquid H2O is produced in this reaction -HCl is a reactant in this equation -the MnCl2 produced is dissolved in water -4.00 g of HCl reacts with 1.00 g of MnO2 -the MnO2 used in this reaction is a solution

-HCl is a reactant in this equation -the MnCl2 produced is dissolved in water

given the balanced equation 3H2(g) + N2(g) --> 2NH3(g), calculate the mass of NH3 produced by the complete reaction of 2.55 g of H2

14.4 g

when hydrogen gas is passed over powdered iron (III) oxide, iron metal and water vapor are formed. give the correct balanced equation for this process

3H2(g) + Fe2O3(s) --> 2Fe(s) + 3H2O(g)

a particular reaction is expected to yield 125 g of calcium. the actual amount of calcium obtained is equal to 105 g. calculate the percent yield for the reaction

84.0%

balance the following equation: Al2S3(s) + H2O(l) --> Al(OH)3(aq) + H2S(g)

Al2S3(s) + 6H2O(l) --> 2Al(OH)3(aq) + 3H2S(g)

what is the actual yield?

amount of product obtained experimentally from a chemical reaction

in order to calculate the overall % yield for a multistep process _____

multiply the individual % yields by each other

What is theoretical yield?

the amount of product calculated from the molar ratio in the balanced chemical equation

which of the following statements describe the information that can be gained from a balanced chemical equation? select all that apply -the identities of substances involved -how fast a given reaction proceeds -the temperature at which a reaction is carried out -the physical states of reactants and products, often -the relative quantities (moles) of substances involved

the identities of substances involved ; the relative quantities (moles) of substances involved

a useful method for keeping track of quantities in a chemical reaction is a reaction table. which of the following are components of a reaction table? select all that apply -final amount of reactants and products remaining after the reaction -initial amounts of reactants and products before reaction -change in the amounts of reactants and products during the reaction -a balanced chemical equation -calculation showing which reactant is limiting

-final amount of reactants and products remaining after the reaction -initial amounts of reactants and products before reaction -change in the amounts of reactants and products during the reaction -a balanced chemical equation

which of the following actions are permitted in balancing a chemical equation? select all that apply -adding reactants or products -inserting coefficients in front of formulas or reactants and products -multiplying all coefficients by a common factor -altering the formula of reactants or products

-inserting coefficients in front of formulas or reactants and products -multiplying all coefficients by a common factor

hydrogen and nitrogen react to form ammonia according to the balanced equation 3H2(g) + N2(g) --> 2NH3(g). in a particular reaction vessel, 4.5 mol of H2 are reacted with 4.5 mol of N2. which of the following options correctly describe how to complete the reaction table given? initial 3H2 : 4.50 moles changed 3H2 : -4.50 moles final 3H2 : 0 initial N2 : 4.50 moles changed N2 : a final N2 : x initial 2NH3 : 0 changed 2NH3 : b final 2NH3: y -the final quantity of NH3 present is 3.0 mole -the quantity of x equals the amount of N2 that reacts -the change in moles of NH3 (b) is equal to +4.5 -the final quantity of N2 present is 0 mol -the change in moles of N2 (a) is equal to -1.5

-the final quantity of NH3 present is 3.0 mole -the change in moles of N2 (a) is equal to -1.5

iodine trichloride is produced in a two step process, represented by the following balanced equations: I2 (s) + Cl2(g)-->2ICl (s) and ICl (s) + Cl2(g) -->ICl3 (s) select all the statements that correctly describe how to write a complete balanced equation for the overall process -the first equation must be multiplied by 2 -the overall equation is given by I2 (s) + 3Cl2(g)-->2ICl3(s) -the second equation must be multiplied by 2 -the overall equation is given by I2(s) +2Cl2(g) + 2ICl(s) --> 2ICl3(s) -the second equation must be subtracted from the first

-the overall equation is given by I2 (s) + 3Cl2(g)-->2ICl3(s) -the second equation must be multiplied by 2

which of the following statements correctly describes the steps used to determine which reactant in a given reaction is limiting? select all that apply -the reactant that has the greatest mass at the beginning of the reaction is in excess -the maximum product possible is given by the sum of the amounts of product formed from each reactant -the reactant that produces the least amount of possible product is the limiting reactant -calculate the molar masses of any reactants for which a mass has been given -calculate the amount of product that could be formed from each reactant

-the reactant that produces the least amount of possible product is the limiting reactant -calculate the molar masses of any reactants for which a mass has been given -calculate the amount of product that could be formed from each reactant

correctly order the steps necessary to solve for the mass of a product, or second reactant required, given the mass of one of the reactants in a chemical process.

-write a balanced equation for the reaction -convert the given mass into moles using molar mass. convert moles of A to moles of B using a conversion factor derived from the balanced equation -convert the moles of the second substance to mass using its molar mass

give the correct steps in order to balance a chemical equation

-write a skeleton equation -balance the atoms -adjust the coefficients such that they are the smallest whole number coefficients -do a final check to make sure the equation is balacned

the compounds depicted are ________ isomers because they have the same ______ formula but have different ______ formulas

functional ; molecular ; structural

what are the 4 symbols used to determine the physical state of a element in a chemical formula?

gas (g), liquid (l), solid (s) and aqueous (aq)

the _____ reactant in a reaction is one that limits the amount of product formed. this reagent will be completely used up in the reaction. any reagents that are not used up are said to be in _____

limiting ; excess