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Which ions is the limiting reagent and which is the reagent in excess when barium sulphate is made?
Wiki User
∙ 9y ago
The ion sulfate (SO4)2- is the limiting reagent.
Wiki User
∙ 8y ago
When barium sulfate is made, the limiting reagent is the one that is completely consumed in the reaction and determines the amount of product formed. In this case, if barium ions (Ba2+) and sulfate ions (SO42−) are the reactants, the limiting reagent would be the one that is present in lower molar quantity. The one in excess would be the one that is present in higher molar quantity. Without the quantities of each ion provided, it is difficult to determine which is the limiting reagent and which is in excess.
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Why excess barium chloride is added to the filtrate in the preparation of a dry sample of barium sulphate?
Barium chloride in excess is added to be sure that the reaction is complete.
3.5 moles of TiCl4 reacts with 4.5 moles of O2 limiting and excess reactants are?
TiCl4 is limiting reagent, O2 is in excess
What is the limiting reactant reagent and what is excess reagent in recrystallization?
The Limiting Reactant is the smaller number once you compare the two reactants with one product. The product that you are comparing them both with must be the same. The Excess Reactant is the larger number, or the amount left over in the chemical reaction.
Can the mass of the limiting reagent be higher than the mass of the excess reagent?
it may be , the limiting reactant is that which is totally consumed during the reaction but its amount must be less than required amount with respect to excess reactant for example, H2SO4 + 2NaOH = Na2SO4 + 2H2O in this reaction suppose acid is 95 g and base is 85 g but acid with higher amount is the limiting reactant and base is in excess. Essentially, it's possible whenever the molecular weight of the limiting reagent is higher than the molecular weights of the other reagents.
When Ammonium Hydroxide excess is added to ferrous sulphate?
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Why excess barium chloride is added to the filtrate in the preparation of a dry sample of barium sulphate?
Barium chloride in excess is added to be sure that the reaction is complete.
3.5 moles of TiCl4 reacts with 4.5 moles of O2 limiting and excess reactants are?
TiCl4 is limiting reagent, O2 is in excess
How do you calculate the percent yield of an element in a reaction?
The actual yield is given within the worded problem. The theoretical yield however is to be found. In order to calculate the theoretical yield, you need to convert the mass of the limiting reagent (LR) to the mass of the reagent in excess (ER). To find the limiting reagent, you need to first convert the mass of the limiting reagent to the mass of the reagent in excess (to find the theoretical yield)A. Convert mass of limiting reagent to mass reagent in excess (mass --> mass); in other words, find the mass of the reagent consumed.1. Multiply the mass of the limiting reagent by the # molecules of the reagent in excess and its molar mass.2. Divide the above by the # of molecules LR which is multiplied by its molar mass.Mass LR x # molecules ER x molar mass ER-- # molecules LR x molar mass LR3. Subtract the original mass of reagent in excess and the consumed reagent in excess.Original mass Reagent in Excess - Consumed Reagent in Excess= Reagent leftover/unused (theoretical yield).B. Find the percent yield of the product.--- Actual YieldTheoretical Yield x 100%
What is a excess reagent?
In most reactions there are two types of reactant. One of them is completely consumed and the other is only partially consumed. The reactant that is only partially consumed is the excess reactant.
Can there be a limiting reagent if only one reagent is present?
The one that runs out first in a reaction - is thoroughly accurate. There are quite a few other limiting reagents in limiting reactions - as well.
What is the limiting reactant reagent and what is excess reagent in recrystallization?
The Limiting Reactant is the smaller number once you compare the two reactants with one product. The product that you are comparing them both with must be the same. The Excess Reactant is the larger number, or the amount left over in the chemical reaction.
Does the excess reagent determine the amount of a product?
The limiting reagent is the determinant because you can only make as much as the smallest amount can provide to react with
How do you test for sulphate ions?
add barium chloride or barium nitrate to a solution containing sulphate ions SO4 2-. To the same solution add hydrochloric acid in excess. OBSERVATIONS, a white precipitate which is insoluble in excess acid confirms presence of SO42- IF IT DISSOLVES then it confirms SO32- ----------------------------------------- 1) Add barium nitrate solution under acidic conditions (use an equal volume of hydrochloric acid) to the unknown solution 2) A white precipitate of barium sulphate forms if sulphate ions are present
Can the mass of the limiting reagent be higher than the mass of the excess reagent?
it may be , the limiting reactant is that which is totally consumed during the reaction but its amount must be less than required amount with respect to excess reactant for example, H2SO4 + 2NaOH = Na2SO4 + 2H2O in this reaction suppose acid is 95 g and base is 85 g but acid with higher amount is the limiting reactant and base is in excess. Essentially, it's possible whenever the molecular weight of the limiting reagent is higher than the molecular weights of the other reagents.
What is the limiting reagent when 3.1 moles of so2 react with 2.7 moles of o2?
2SO2 +O2 -----> 2SO3 so 3.1 moles of SO2 would require 1.55 moles of O2 so since there are 2.7 moles of O2 present and thus in excess, the SO2 is the limiting reagent.
What steps are needed to determine the amount of excess reagent in a chemical reaction?
To determine the amount of excess reagent in a chemical reaction, first calculate theoretical values for your reaction to get an estimation of how much of your excess reagent will be left once the limiting reagent is used. Then run the actual experiment and measure!
Conversions of stoichiometry?
Stoichiometry Conversions Using Balanced EquationsMol A --> Mol B (Mol -->Mol)("How many moles of B are needed to react with X mol A?") __A + __B --> __AB1. Multiply the number of moles (A) by the number of moles (# molecules)1 for B.2. Divide the result by the number of molecules for A.- FormulaMol A * # molecules B/# molecules A- Conversion factorMol A * # molecules (mol) B = Mol B----- # molecules (mol) A*****1 the number of moles in this case refers to however many molecules of each substance is within the balanced equation (# molecules). For clarity sake I put # molecules in place of "moles" where appropriate; however, on practice problems or demonstrations shown in textbooks, it's likely it will say moles instead of # molecules.*****Mol A --> Mass B (Mol --> Mass)("How many grams B are needed to produce X mol A?") __A + __B --> __AB1. Multiply mol A by # molecules B; divide by # molecules A. (Mol A --> Mol B)2. Multiply result from 1 by molar mass B (mol B --> Mass B).- FormulaMol A x # molecules B/# molecules A- Conversion FactorMol A x # molecules (mol) B x molar mass B = mass B--------- # molecules (mol) A ----- 1 mol BMass A --> Mol B (Mass --> Mol)("How many mol of B are needed to react with X g A?") __A + __B --> __AB1. Multiply Mass A by # molecules B.2. Divide by molar mass multiplied by # molecules A.- FormulaMass A x # molecules B/(Molar Mass A x # molecules A)- Conversion FactorMass A x 1 mol A x # molecules (mol) B = mol B--- molar mass A - # molecules (mol) AMass A --> Mass B (Mass --> Mol --> Mass)("How many grams of A can be produced from X grams B?") __A + __B --> __AB1. Convert from grams (g) to mol for substance A (mass A --> mol A).2. Divide mol A by mol B (mol A --> mol B [Molar Ratio of Substances]).3. Multiply mol B by molar mass B (mol --> mass)In summary, you are converting from grams A to mol A, then mol A to mol B, then mol B to grams B.- FormulaMass A x # molecules B x Molar Mass B/(Molar Mass A x # molecules A)- Conversion FactorMass (g) A * 1 mol A -- x -- # molecules (mol) B -- x -- molar mass B = mass B----- molar mass (g) A --x-- # molecules (mol) A --- x --- 1 mol BLimiting Reagent and Reagent in ExcessThe limiting reagent or limiting reactant is the substance that limits the reaction. ("What substance has the least amount produced from a reaction?"). The reagent in excess or reactant in excess is the product left over or reagent that is leftover from the reaction; in other words, the reagent that has the most product that did not react.To identify the limiting reagent or limiting reactant, identify which substance produced the least amount of product (which reactant yields the least amount of product).Steps (given masses of products):A. Identify amount of product created per reactant (reactant --> product yield).1. Balance the equation if it has not been done already.2. Convert the given masses of reactant (A, B, etc.) to mass product (C) (see "Mass A --> Mass B [Mass --> Mass]" above). (mass reagent --> mass product)B. Identify the limiting reagent. The limiting reagent (reactant) will be the reactant (A, B, etc.) that yields the least amount of C (product).C. Identify the reagent in excess. The reagent in excess (reactant) will be the reactant (A, B, etc.) that yields the most amount of C (product).D. Give how much reagent in excess remain unreacted. (How much reactant is leftover). For simplicity sakes, the limiting reagent will be A and the reagent in excess will be B. "For every X grams of the limiting reagent, there is Y grams of the reagent in excess".Mass Limiting Reactant --> Mass Reagent in Excess:First convert the mass of the limiting reagent to the mass of the reagent in excess (mass limiting reagent : mass reagent in excess [reacting] ratio); then subtract the mass of the limiting reagent from the mass of the reagent in excess (that reacted)1. Convert the mass of the limiting reagent to mass of the reagent in excess (ratio mass limiting reagent: mass reagent in excess). Refer to "Mass A --> Mass B" above.2. Subtract the original amount of B (reagent in excess) from the amount of B needed to react with A (limiting reagent).Reagent in Excess leftover = Starting Mass A - Reacting Mass B (step 1 answer)E. Find % yield.% yield = actual yield (given)------- theoretical yield (must be found)** the theoretical yield is the amount of product theoretically produced by the limiting reagent; the actual yield is the amount of product actually produced by the reactants; the theoretical yield will have been found in step A. The actual yield will be given within the worded problem.Ex. 4Na2CO3 + Fe3Br8 --> 8NaBr + 4CO2 + Fe3O4 A. How many grams of Fe3O4 can be produced from 100.0g Na2CO3 and 300.0g Fe3Br8?100.0g Na2CO3 x 1 mol Na2CO3 x 1 mol Fe3O4 x 231.6g Fe3O4------------------ 106.0g Na2CO3 -- 4 mol Na2CO3 -- 1 mol Fe3O4= 54.62g Fe3O42(2 this is known as the theoretical yield, which will be needed when calculating percentage yield later on).300.0g Fe3Br8 x 1 mol Na2CO3 x 1 molecules Fe3O4 x 231.6g Fe3O4----------------- 106.0g Fe3Br8 ---- 4 molecules Fe3Br8 -- 1 mol Fe3O4= 86.12g Fe3O4B. What is the limiting reagent?The limiting reagent in this case is Na2CO3 because it has the lowest theoretical yield for producing Fe3O4 (54.62g Fe3O4 vs 86.12g Fe3O4).C. What is the reagent in excess?The reagent in excess is Fe3Br8 because it has the highest theoretical yield for producing Fe3O4.D. How many grams of the reagent in excess(Fe3Br8)remain unreacted?100.0g Na2CO3 x 1 mol Na2CO3 x 1 molecules Fe3Br8 x 806.8g Fe3Br8------------------- 106.0g Na2CO3 -- 4 molecules Na2CO3 - 1 mol Fe3Br8= 190.3g Fe3Br8300.0g Fe3Br8 - 190.3g Fe3Br8 = 109.7g Fe3Br8 leftover (unreacted)E. If 42.75g of Fe3O4 were isolated, what is the % yield?% yield = 42.75g----------- 54.62g2 x 100% = 78.27%
