Answered: D are products. How many moles of D can…

D are products. How many moles of D can be produced with 5.98 moles of A being completely reacted? Use mol as the unit and keep correct number of significant figures. 3 A + 2 B -----> 4 C+ 2 D

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter3: Stoichiometry

Section: Chapter Questions

Problem 36Q: Consider the following generic reaction: Y2+2XY2XY2 In a limiting reactant problem, a certain...

See similar textbooks

Related questions

Q: Consider the following unbalanced chemical equation. CSH12() + O2(g) → CO2(g) + H20(1) If 46.1 grams…

Q: The balanced chemical equation for the reaction between aluminum oxide and sulfuric acid is:…

A: The given chemical reaction between aluminum oxide and sulfuric acid is,…

Q: How many moles of magnesium oxide are produced from 4.34x10^24 particles of magnesium? (round to the…

A: Number of moles of Magnesium

Q: How many moles of potassium ions are in 360. g alum? (b) What is the mass % S in alum (to 3…

Q: Ethylene (C₂H4) reacts with molecular hydrogen according to the equation below. C2H4 (g) + H2 (g)…

A: The given reaction is: C2H4 (g) + H2 (g) --> C2H6 (g) Molar mass of C2H4 (g)= 28.05 g/mol Molar…

Q: Percent yield of chemical reactions O 1/5 Gaseous methane (CH) reacts with gaseous oxygen gas (0,)…

Q: Which is the correctly balanced form of the given equation? S(s) + O3(g) SO2(g)a) S(s) + O3(g)…

A: A chemical reaction equation which contains same number of atoms on both reactant and product side…

Q: 1A. Consider the balanced chemical equation that follows: 2Fe(s) + 3S(s) → Fe2S3(s) This equation…

Q: 5. Benzene, C&H6, has a density of 0.787 g/mL. Burning 10.0 mL of benzene would produce how many…

Q: Silicon to be used in computer chips is manufactured in a process represented bythe following…

Q: Consider the following unbalanced reaction: P4 (s)+F2(g)→ PF3 (g) What mass of F2 is needed to…

Q: N2(g) + 3H2(g) —> 2NH3(g) What mass in grams of Ammonia (NH3) is produced from 25 moles of Hydrogen…

A: Given reaction is N2(g) + 3H2(g) -------> 2NH3(g) Moles of hydrogen = 25 moles Molar mass of…

Q: Diesel Fuel C14.4H24.9 is burned with atmospheric air in a stoichiometric ratio. The total number of…

A: Given diesel fuel : C14.4H24.9 is burned in air in stoichiometric ratio.

Q: 8. Consider the reaction: MnO2 + 4HCI → MnCl2 + Cl2 + 2H20 If 0.86 mole of Mn02 and 48.2 g of HCl…

A: 1- Calculate the moles of HCl first : moles of HCl = ( mass / molar mass of HCl ) moles of HCl = (…

Q: In the lab, 9.00 g of hydrogen, H2, is reacted with excess oxygen gas, O2, and 73.0 g of water is…

Q: When elemental carbon is burned in the open atmosphere, with plenty of oxygen gas present, the…

Q: 3 a. Rewrite the balanced equation, if necessary, using CuCl2 as the formula for copper chloride.…

Q: Consider the following reaction for Pentane (C5H12): C5H12 + 8O2 --> 5CO2 + 6H2O If 2.5 moles of…

A: On reaction completion, one of the reactants is always left unconsumed, while the other is totally…

Q: Methanol can be formed by the following UNBALANCED equation below. What is the mass in grams of…

A: First one need to balance the equation 2H2(g) + CO(g) →CH3OH(l) Now mole Concept need to applied.

Q: Liquid octane (CH3(CH,) CH, reacts with gaseous oxygen gas (0,) to produce gaseous carbon dioxide…

Q: How many grams of H2O are formed from the complete reaction of 32 g of O2 according to this…

A: Hydrogen reacts with oxygen to form water. The equation for the balanced chemical reaction is as…

Q: Question attached

A: Number of moles of the substance is equal to the ratio of mass to the molar mass of the substance.…

Q: Silicon tetrachloride (SiCl4 ) can be prepared by heating Si in chlorine gas: Si(s) + 2Cl2(g) ->…

A: Molar mass of Cl2 = 70.9 g/mol

Q: A complete combustion of octane, C8H18, a component of gasoline, proceeds as: 2 C8H18(I) +25 O2(g)…

Q: How many moles (of molecules or formula units) are in each sample? 0.2011 g C8H18 Express your…

A: Given, mass of C8H18 = 0.2011 g Molar mass of C8H18 = 114.23 g/mol

Q: Methanol can be formed by the following UNBALANCED equation below. What is the mass in grams of…

A: The given unbalanced chemical reaction is: H2g+COg→CH3OHl The balanced form of this reaction is:…

Q: H2SO4(aq) + Pb(C2H3O2)2(aq) --> PBSO4(s) + 2 HC2H3O2(aq) Solutions of sulfuric acid and lead (II)…

A: A reaction between H2SO4 and Lead acetate, which gives Lead sulphate and acetic acid.

Q: When the equation AgNO3 + MgCl2 ----> AgCl + Mg(NO3)2 is completely balanced with the smallest whole…

A: Given unbalanced equation is AgNO3 + MgCl2 = AgCl + Mg(NO3)2

Q: (a) How many moles of C atoms are in 1 mol of sucrose (C12H22011)? (1 mol is an exact number.) mol C…

A: (a) • The values provided in the question are:- i) Number of moles of sucrose= 1 mol •…

Q: 2H2(g) + O2 (g) —> 2H2O (I) What mass in grams of Water (H2O) is produced from 2 moles of Hydrogen…

A: 2 moles of hydrogen forms 2 moles of water

Q: 2 N2O5 ----> 4 NO2 + O2 What mass of NO2 can be produced from the complete reaction of 38.2 g of…

A: Given Reaction 2N2O5 → 4NO2 + O2 Mass of N2O5 = 38.2 gram Mass of NO2 = ?

Q: Citric acid (C6H3O7), named for its natural occurrence in citrus fruits, is produced in large…

A: Given; C12H22O11 + 3O2 ➝ 2C6H8O7 + 3H2O Note: (1Kg = 1000g) Mass of sucrose (C12H22O11) = 600.0 Kg =…

Q: For the chemical reaction 2Al + 3H2SO4---> 3H2+ Al2(SO4)3 how many moles of hydrogen will be…

Q: 22. The combustion of hexane (C,H14), a component of gasoline, is represented by the balanced…

A: A combustion reaction of hexane. Balanced chemical Reaction :- 2C6H12 (l) + 19O2 (g) --> 12CO2…

Q: H2SO4(aq) + Pb(C2H302)2(aq) --> PbSO4(s) + 2 HC2H302(aq) Solutions of sulfuric acid and lead (II)…

A: The balanced reaction is – H2SO4 aq+ PbC2H3O2 aq→PbSO4 aq+2HC2H3O2aq

Q: Consider the following unbalanced chemical equation. C5H12(1) + O2(g) → CO2(g) + H20(1) If 19.2…

A: Recall, the unbalanced chemical equation, C5H12 (l) + O2 (g) CO2 (g) +…

Q: The Haber-Bosch process involves the combination of nitrogen and hydrogen at high temperatures in…

Q: 1. A sample of 25.3 grams of BaSO, is mixed with 18.6 grams of Na3PO4- A) Determine which is the…

Q: Liquid octane (CH3 (CH2),CH;)' reacts with gaseous oxygen gas (02) to produce gaseous carbon dioxide…

A: The percentage yield is the ratio of the actual yield to the theoretical yield, multiplied by 100…

Q: Gaseous bulane(-3-2/2 ,CH3) will react with gaseous oxygen (0)) to produce gaseous carbon dioxide…

A: Balanced equation: 2C4H10 (g) + 13O2 (g) --------> 8CO2 (g) + 10H2O (g) Number of mols…

Q: 3. Mass Ratio. Hydrogen gas for fuel cells can be made by decomposing methane (CH4), which is the…

Q: Balance chemical equation given below. HoW much lithium nitride is produced when 20 g of lithium and…

A: In Balanced chemical equation number of atoms of each species are equal on both reactant and…

Q: Liquid octane (CHa (LH2)6 CH.) will react with gaseous oxygen (0)) to produce gaseous carbon dioxide…

Q: Citric acid (C6H$O7), named for its natural occurrence in citrus fruits, is produced in large…

A: Citric acid named for its natural occurrence in citrus fruits, is produced in large quantities…

Q: Consider the balanced chemical reaction below. What is the maximum amount of grams of Fe that can be…

A: Given: Mass of Iron(III) Oxide 33.4 g Mass of Carbon monoxide= 47.2 g To find: Mass of Fe produced…

Q: A student heats a 2.8695g sample of a mixture that contains an unknown amount of potassium chlorate…

A: Given: Mass of sample sample = 2.8695 g And mass of residue after heating = 2.0427 g

Q: Fernando is doing his pre-lab homework for Chemistry. He is asked to predict how many grams of CO2…

A: Given Reaction is - CaCO3 + 2HCl ----> CaCl2 + CO2 + H2O The calculated theoretical yield of…

Q: Sulfuric acid reacts with aluminum hydroxide according to the reaction 3 H2SO4 + 2 Al(OH)3 --->…

Q: DDT, an insecticide harmful to fish, birds and humans, is produced by the following reaction 2C6H5Cl…

A: Since you have posted multiple questions, we are entitled to answer the first only.

Concept explainers

Ionic Equilibrium

Chemical equilibrium and ionic equilibrium are two major concepts in chemistry. Ionic equilibrium deals with the equilibrium involved in an ionization process while chemical equilibrium deals with the equilibrium during a chemical change. Ionic equilibrium is established between the ions and unionized species in a system. Understanding the concept of ionic equilibrium is very important to answer the questions related to certain chemical reactions in chemistry.

Arrhenius Acid

Arrhenius acid act as a good electrolyte as it dissociates to its respective ions in the aqueous solutions. Keeping it similar to the general acid properties, Arrhenius acid also neutralizes bases and turns litmus paper into red.

Bronsted Lowry Base In Inorganic Chemistry

Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.

Question

In a balanced generic reaction below, letters A and B represent reactant while C and
D are products. How many moles of D can be produced with 5.98 moles of A being
completely reacted? Use mol as the unit and keep correct number of significant
figures.
3 A+ 2 B -----> 4 C+ 2 D

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Answer

VIEW

Step by step

Solved in 3 steps

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

What is meant by a limiting reactant in a particular reaction? In what way is the reaction “limited”? What does it mean to say that one or more of the reactants are present in excess? What happens to a reaction when the limiting reactant is used up?
Consider the equation: 2A+B5C. If 10.0 g of A reacts with 5.00 g of B. how is the limiting reactant determined? Choose the best answer and explain. l type='a'> Choose the reactant with the smallest coefficient in the balanced chemical equation. So in this case, the limiting reactant is B. Choose the reactant with the smallest mass given. So in this case, the limiting reactant is The mass of each reactant must be converted to moles and then compared to the ratios in the balanced chemical equation. So in this case, the limiting reactant cannot be determined without the molar masses of A and B. The mass of each reactant must he converted to moles first. The reactant with the fewest moles present is the limiting reactant. So in this case, the limiting reactant cannot be determined without the molar masses of A and B. The mass of each reactant must be divided by their coefficients in the balanced chemical equation, and the smallest number present is the limiting reactant. So in this case, there is no limiting reactant because A and B arc used up perfectly.
4.72 The picture shown depicts the species present at the start of a combustion reaction between methane, CH4 and oxygen, O2 (a) What is the limiting reactant? (b) Draw the resulting state after this set of reactants has reacted as far as possible.
The pictures below show a molecular-scale view of a chemical reaction between H2 and CO to produce methanol, CH3OH The box on the left represents the reactants at the instant of mixing, and the box on the right shows what is left once the reaction has gone to completion. D Was there a limiting reactant in this reaction? If so, what was it? Write a balanced chemical equation for this reaction. As usual, your equation should use the smallest possible whole number coefficients for all substances.
Explain how one determines which reactant in a process is the limiting reactant. Does this depend only on the masses of the reactant present? Give an example of how to determine the limiting reactant by using a Before-Change-After (RCA) table with a balanced chemical equation and reactant starling amounts.
For each of the following balanced reactions, calculate how many moles of each product would be produced by complete conversion of 0.50 mole of the reactant indicated in boldface. Indicate clearly the mole ratio used for the conversion. msp;2H2O(l)2H2O(l)+O2(g) msp;2KClO3(s)2KCl(s)+3O2(g) msp;2Al(s)+6HCl(aq)2AlCl3(aq)+3H2(g) msp;C3H8(g)+5O2(g)3CO2(g)+4H2O(g)
Consider the following generic reaction: Y2+2XY2XY2 In a limiting reactant problem, a certain quantity of each reactant is given and you are usually asked to calculate the mass of product formed. If 10.0 g of Y2 is reacted with 10.0 g of XY, outline two methods you could use to determine which reactant is limiting (runs out first) and thus determines the mass of product formed.
For each of the following unbalanced reactions, suppose exactly 5.00 g of each reactant is taken. Determine which reactant is limiting, and also determine what mass of the excess reagent will remain after the limiting reactant is consumed. Na2B4O7(s) + H2SO4(o H3BOj(j) + Na2SO4(u CaC,(s) + H2O(/) Ca(OH)2(s) + C2H2(g) NaCl(s) + H2SO4(/> HCl(g) + Na2SO4(s) SiO2(s) + C(x) —> Si(/) + CO(g)
4.71 The particulate scale drawing shown depict the products of a reaction between N2 and O2 molecules. (a) Draw a similar representation for the reactants that must have been present before the reaction took place. (b) Write a balanced chemical equation for the reaction, using the smallest possible whole number coefficients. (c) Identify the limiting reactant, and explain how the pictures allow you to do so.
4.70 The particulate scale drawing shown depicts the products of a reaction between H2 and O2 molecules. (a) Draw a similar representation for the reactants that must have been present before the reaction took place. (b) Write a balanced chemical equation for the reaction, using the smallest possible whole number coefficients. (c) identify the limiting reactant, and explain how the pictures allow you to do so.
For each of the following unbalanced chemical equations, suppose exactly 5.0 g of each reactant is taken. Determine which reactant is limiting, and calculate what mass of each product is expected, assuming that the limiting reactant is completely consumed. msp;Na(s)+Br2(l)NaBr(s) msp;Zn(s)+CuSO4(aq)ZnSO4(aq)+Cu(s) msp;NH4Cl(aq)+NaOH(aq)NH3(g)+H2O(l)+NaCl(aq) msp;Fe2O3(s)+CO(g)Fe(s)+CO2(g)
For each of the following incomplete and unbalanced equations, indicate how many moles of the second reactant would be required to react completely with 0. 145 mole of the first reactant. msp;BaCl2(aq)+H2SO4(aq) msp;AgNO3(aq)+NaCl(aq) msp;Pb(NO3)2(aq)+Na2CO3(aq) msp;C3H8(g)+O2(g)