Question

ORT ui jo ssaoxa uan pea o ape aam EHN Jou 00E0 9.ON Cos.HN jou 00'E (C anoqe aua jo auou (3 B) The percent yield %001 limiting reagent. (2 es an n apanpoad A e npoad jo aunoue a rene 24) Consider the following generic chemical equation: 2W +3X+3Y+Z maes anu aue anoqe ap jo IIV ( 3o unoue aup uo paseq apeu aq ues jep npoud jo junouue a sl pl e auoa a ( X (V M (B Z (a (2 25) A balanced chemical equation used to prepare ammonium carbonate, (NH4)2CO3, is: 2 NH3 CO2 H20 (NH4)2CO3 A) React 2 moles NH, 8 moles CO2, and 8 moles H2O B) React 2 moles NH3, 1 mole CO2, and 1 mole H2O C) React 4 moles NH3, 1 mole CO2, and 2 moles HyO (20 D) React 4 moles NH3, 2 moles CO2, and 2 moles H2O jo unoue saas ap u insau pinoM Mojaq umous sappuenb juepeau jo aop n 26) What is the theoretical yield of a reaction if 25.0 grams of product were actually produced from a anoqe aup o auou (3 reaction that has a 88% yield ? E) none of the above (92

Answer 1

answer22) A) 4.50 mol

4NH₃ +5O₂ ---->4NO + 6H₂O

Given 3.00 mol of NH₃ used woth excess of O₂ , so ammonia is the limiting reagent . The amount of products formed is only dependent upon ammonia.

From above balanced chemical reaction ,

4 mol of ammonia gives 6 mol water

1 mol of ammonia gives 6/4 mol of water

1 mol of ammonia gives 1.5 mol of water

Given is 3.00 mol of ammonia

3.00 mol of ammonia gives 1.5 × 3.00 mol of water

3.00 mol of ammonia gives 4.50 mol of water

answer23)E) All of the above are true statements

the actual yield is the amount of product actually produced by a chemical reaction. ( true )

the percent yield equal to actual yield divided by theoretical yield multipled by 100. (True)

limiting reactant is the completely consumed in a chemical reaction. (True) because limiting reactant is present in the least amount so is consumed completely

the theoretical yield is the amount of product that can be made based on the amount of limiting reagent.

answer24) X

2W + 3X --->3Y + Z

Given : 5 units of W and 6 units of X

From the above balanced chemical reaction

2 units of W reacts with 3 units of X

So ,1 units of W reacts with 3 ÷ 2 units of X

1 units of W reacts with 1.5 units of X

Given is 5 units of W

5 units of W reacts with 5 × 1.5 units of X

5 units of W reacts with 7.5 units of X

But given amount of X is 6 units , therefore X is the limiting reactant and W is in excess .

answer25) D) react 4 moles NH_{3 ,}2 moles CO₂ ,and 2 moles H₂O

The molar ratio of reactants in given balanced chemical reaction is

NH₃ : CO₂ : H₂O = 2 : 1 : 1

In part A) ratio is 2 : 8 : 8 , so NH₃ is the limiting reactant because least in amount

And it(2 mol of ammonia) thus gives 1 mol of product according to balanced chemical reaction.

In part B) ratio is 2 : 1 : 1

None of them are limiting reactant because all are present same as in the balanced chemical reaction , so amount of product can be calculated from any of the given reactants.

And so gives 1 mol of H₂O gives 1 mol of product

In part C) ratio is 4: 1: 2

Here CO₂ is the limiting reactant

So 1 mol CO₂ gives 1 mol of product

In part D) ratio is 4: 2 : 2

None of them are limiting reagent because all are present in same ratio(4:2:2=2:1:1) as given in the balanced chemical reaction so any of them can be used to predict the amount of product formed.

So 2 mol of CO₂ gives 2 mol of product formed.