Limiting Reactants flashcards

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what is a limiting reaction? This is a chemical reactant that limits the product formed in a reaction
what are limiting reagents used for? The limiting reagent gives the smallest yield of the product which can be calculated from the reagents
what is a product? A product is the compound that is created when a chemical reaction occurs
what is a reactant? it is a substance that participates in a chemical reaction
what happens when you limit a reaction? there will be a limited amount of product that is produced
when does a chemical reaction stop? it stops when the reactant are used up
In a reaction, the amount of product is directly proportional to the amount of the limiting reactant
If 4.95 g of ethylene (C2H4) are combusted with 3.25 g of oxygen. what is the limiting reagent? O2
2H2 + O2 --> 2H2O | 10.0 grams of hydrogen and 15.0 grams of oxygen. what is the limiting reactant? Oxygen is limiting reactant, as the amount of H2O is much less than that produced by hydrogen
HCl + NaOH --> NaCl + H2O | if there are 37g HCl and 60g NaOH present. what is the limiting reactant? HCl is the limiting reactant.
Determine the limiting reactant (LR) and the mass (in g) of nitrogen that can be formed from 50.0 g N2O4 and 45.0 g N2H4.
N2O4(l) + 2N2H4(l) => 3N2(g) + 4H2O(g)
LR = N2O4, 45.7 g N2formed
what are excess reactants? This is the reactant that remains when a reaction stops, once the limiting reactant is consumed
NH3 + O2 NO + H2O. | 3.25 g of NH3 react with 3.50 g of O2, how much excess reactant remain 1.76 g NH3 left
What is actual yield? This is the actual yield of the product in grams that is formed
what is the actual yield formula (percent yield x theoretical yield) / 100%
what is theoretical yield? This is the yield of the product in gram formed from the limiting reagent
what is the formula for theoretical yield? actual yield / percent yield x 100%
LiOH + KCl --> LiCl + KOH | given 20g LiOH, what is the theoretical yield? 16.9%
Determine the theoretical yield of HCl if 60.0 g of BCl3 and 37.5 g of H2O are reacted according to the following balanced reaction.
BCl3(g) + 3H2O(l) => H3BO3(s) + 3HCl(g)
56.0 g HCl
what is percentage yield? This gives the yield of the product as a percentage based on the theoretical yield
what is the formula for percentage yield? % yield = actual yield / theoretical yield x 100
C6H6 + Br2 C6H5Br + HBr. If actual yield of C6H5Br is 63.6 g, what is the percent yield? 88.6%
what is the % yield of water if 138g H20 is produced from 16g H2 and excess O2? % yield = actual/theoretical x 100% = 138g H2O/142g H2O x 100% = 96.7%
Identify the percent yield when 28.16 g of CO2 are formed from the reaction of 4.000 moles of C8H18 with 4.000 moles of O2.
2C8H18 + 25O2 => 16CO2 + 18H2O
25.00%

what is a limiting reaction?

what are limiting reagents used for?

what is a product?

what is a reactant?

what happens when you limit a reaction?

when does a chemical reaction stop?

In a reaction, the amount of product is directly proportional to the amount of the

If 4.95 g of ethylene (C2H4) are combusted with 3.25 g of oxygen. what is the limiting reagent?

2H2 + O2 --> 2H2O | 10.0 grams of hydrogen and 15.0 grams of oxygen. what is the limiting reactant?

HCl + NaOH --> NaCl + H2O | if there are 37g HCl and 60g NaOH present. what is the limiting reactant?

Determine the limiting reactant (LR) and the mass (in g) of nitrogen that can be formed from 50.0 g N2O4 and 45.0 g N2H4.
N2O4(l) + 2N2H4(l) => 3N2(g) + 4H2O(g)

what are excess reactants?

NH3 + O2 NO + H2O. | 3.25 g of NH3 react with 3.50 g of O2, how much excess reactant remain

What is actual yield?

what is the actual yield formula

what is theoretical yield?

what is the formula for theoretical yield?

LiOH + KCl --> LiCl + KOH | given 20g LiOH, what is the theoretical yield?

Determine the theoretical yield of HCl if 60.0 g of BCl3 and 37.5 g of H2O are reacted according to the following balanced reaction.
BCl3(g) + 3H2O(l) => H3BO3(s) + 3HCl(g)

what is percentage yield?

what is the formula for percentage yield?

C6H6 + Br2 C6H5Br + HBr. If actual yield of C6H5Br is 63.6 g, what is the percent yield?

what is the % yield of water if 138g H20 is produced from 16g H2 and excess O2?

Identify the percent yield when 28.16 g of CO2 are formed from the reaction of 4.000 moles of C8H18 with 4.000 moles of O2.
2C8H18 + 25O2 => 16CO2 + 18H2O

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