Answered: How many moles of NH3 can be produced…

How many moles of NH3 can be produced from 3.76 moles of nitrogen in the following reaction: N2 (g) + 3 H2 (g) → 2 NH, (g) ->

Introductory Chemistry For Today

8th Edition

ISBN:9781285644561

Author:Seager

Publisher:Seager

Chapter5: Chemical Reactions

Section: Chapter Questions

Problem 5.88E

See similar textbooks

Related questions

Q: How much HNO3 can be formed in the following reaction if 36 g of NO2 gas is bubbled through 25 g of…

Q: A chemist combines 136.4 kg of ammonia with 211.4 kg of carbon dioxide for industrial synthesis of…

A: Calculate the mass of NH3 needed and identify the limiting reactant, mass of NH3…

Q: Silicon nitride (Si3N4), a valuable ceramic, is made by the direct combination of silicon and…

A: Percent yield is defined as the percentage ratio of the actual yield to the theoretical yield…

Q: If you had 6 CO2 molecules and 6 H2O molecules…. How many molecules of C2H4 could you produce?

A: 2CO2 + 2H2O = C2H4 + 3O2

Q: If 3.71 mol of C5H12 reacts with excess O2, how many moles of CO2 will be produced by the following…

A: The balanced reaction taking place is given as, => C5H12 + 8 O2 -------> 5 CO2 + 6 H2O

Q: The equation for the reaction between sodium hydrogen carbonate and sulfuric acid at room…

Q: According to the following balanced reaction, how many moles of NO can be formed from 3.00 moles of…

A: Limiting reactant :- A reactant whose number of moles are less than the number of moles required as…

Q: How many grams of CuO would be required to produce 63.5 moles of nitrogen gas in the following…

A: GIVEN : Reaction: NH₃(g) + 3 CuO(s) → 3 Cu(s) + N₂(g) + 3 H₂O(g) To Solve: Mass of CuO required=?…

Q: Adipic acid, H2C6H8O4, used to produce nylon, is made commercially by a reaction between cyclohexane…

A: The limiting reagent in a chemical reaction is a reactant that is totally consumed when the chemical…

Q: When hydrochloric acid reacts with oxygen, water and chlorine are produced. The balanced equation…

Q: Write the balanced equation, then outline the steps necessary to determine the information requested…

A: Since we only answer up to 3 sub-parts, we’ll answer the first 3. Please resubmit the question and…

Q: What is the mass in grams of NO that will be produced from 19.7 g of NO, reacted with excess water…

Q: How many grams of CuO would be required to produce 10.0 moles of nitrogen gas in the following…

A: Given:

Q: How many grams of sulfur (S) are needed to react completely with 45.0 g of aluminum (Al) in the…

A: Aluminum reacts with sulfur to form aluminum sulfide. The equation for the balanced chemical…

Q: Silicon nitride is synthesized according to the reaction: 3Si(s)+2N2(g)→Si3N4(s) How much Si is…

Q: 892.1 grams of isomaltitol, C12H24O11, was combusted in a furnace completely in an excess oxygen.…

A: The yield of water can be calculated as:-

Q: Industrially, nitric acid is produced by the Ostwald process, as represented by the following…

A: The theoretical yield of a reaction can be calculated as follows. Theoretical yield=actual…

Q: How many grams of H2 can be formed from 87.2 grams of NH3 in the following reaction? 2 NH3(g) 3 H2…

Q: if you have 1 mol Xe and 1 mol F2,how many moles of XeF4 ,can you create in the following chemical…

A: • The given balanced chemical equation is, Xe(g) + 2 F2(g) → XeF4(g) • The…

Q: How many grams of CuO would be required to produce 81.0 moles of nitrogen gas in the following…

A: The reaction available is 2NH3(g) +3CuO(s) →3Cu(s)+N2(g) +3H2O(g)

Q: Aluminum carbide, Al4C3, is a yellow powder that reacts with water to produce aluminum hydroxide and…

Q: 5. Methane (CH) undergoes combustion according the following reaction: CH. (g) + O2 (g) → CO: (g) +…

Q: For the chemical reaction 2NaOH+H2SO4⟶Na2SO4+2H2O, how many moles of sodium sulfate will be produced…

A: 1- First calculate the moles of NaOH : moles of NaOH = ( mass / molar mass of NaOH) moles of NaOH…

Q: In the reaction, CuSO4(aq) + 4 NH3(aq) →Cu(NH3)4SO4(aq) a. What is the theoretical yield if 10.0 g…

Q: The synthesis of maleic acid anhydride (C₄H₂O₃) can be accomplished by reacting benzene (C₆H₆) and…

A: 2 C₆H₆(l) + 9 O₂(g) → 2 C₄H₂O₃(s) + 4 CO₂(g) + 4 H₂O(g) According to the above equation, 9 moles of…

Q: reaction product is produced in a 76.3% yield. If the actual yield of the isolated product is 31.1…

A: Percentage yield= (actual yield/theoretical yield)*100% Let m=theoretical yield 76.3 =(31.1/m)*100…

Q: how many grams of calcium hydroxide, Ca(OH)2, are needed to react completely with 65.9 g of…

A: Given: Mass of HCl = 65.9 g Molar mass of HCl = 36.46 g/mol Molar mass of Ca(OH)2 = 74.092 g/mol

Q: Given the reaction: 4NH3 (g) + 5 O2 (g) → 4 NO (g) + 6 H2O (l) When 1.25 mole of ammonia reacts,…

Q: Ammonia, NH3, is prepared by the following reaction: 2 NO2(g) + 5 H2(g) - 2NH3(g) + 2 H2O(I)…

Q: Industrially, nitric acid is produced by the Ostwald process, as represented by the following…

Q: A sample of a compound of Cl and O reacts with an excess of H2 to give 0.233 g HCl and 0.403 g of…

Q: 1. Consider the production of phosphorus trichloride (PCI,) from phosphorus (P) and chlorine (Cl,)…

Q: 4. What would be the limiting reactant if 9 g of water reacted with sodium to form 0.4g H2?

Q: 3. Which of the following statements is FALSE for the chemical equation given below in which…

Q: Consider the following reaction for formation of nitric acid from the pollutant nitrogen dioxide…

Q: Consider the reaction: 3A+4B -> 3C What is the limiting reactant if 1 mole of A is allowed to…

Q: When elemental phosphorus oxidizes, it produces a covalently bonded molecule known as…

A: Given :- Mass of P4 = 1.33 g Mass of O2 = 5.07 g To calculate :- Theoretical yield of P4O10

Q: What is the mass in grams of H2 that can be formed from 89.6 grams of NH3 in the following reaction?…

Q: Industrial production of hydrogen gas uses the reaction shown below. If 1.00 metric ton of propane…

A: A mole is collection of particle A mole of a substance is equal to the molar mass of substance If…

Q: Given the balanced chemical equation,C4H4 + 5 O2 → 4 CO2 + 2 H2O.How many grams of water can be…

A: The balanced reaction given is C4H4 + 5 O2 → 4 CO2 + 2 H2O. hence we can say that 1 mole of C4H4…

Q: Industrial production of hydrogen gas uses the reaction shown below. If 1.00 metric ton of propane…

A: Theoretical yield :- The maximum amount of the product formed when reactants are consumed as per…

Q: Ethanol, used in alcoholic beverages, can be produced by the fermentation of sucrose, which is found…

A: We can solve the given questions by using unitary method.

Q: One starting material for the preparation of nylon is adipic acid, which is produced from the…

Q: Methanol can be produced through the reaction of CO and H, in the presence of a catalyst. catalyst…

A: Given data Mass of CO reacted 75.0 g CH3OH produce 68.4 g

Q: DDT, an insecticide harmful to fish, birds, and humans, is produced by the following reaction: 2C6H;…

A: Since we only answer up to 3 sub-parts, we’ll answer the first 3. Please resubmit the question and…

Q: What mass of carbon dioxide is produced by the complete combustion of 237 g of the hydrocarbon…

Q: Based on the balanced reaction: 6 CO2 + 6 H2O→ 6 O2 + C6H12O6, what is the maximum number of grams…

A: 6 CO2 + 6 H2O→ 6 O2 + C6H12O6 molecular mass of CO2 = 44g

Q: Pure iron, Fe, can be produced from an ore called hematite, Fe2O3 , by reaction with carbon at high…

A: Given: Mass of iron (Fe) = 47 ton Molar mass of Fe = 55.845 g/mol Molar mass of Fe2O3 = 159.69 g/mol

Q: Determine the limiting reactant and the percent yield of this reaction. How many molecules of…

Concept explainers

Stoichiometry

Stoichiometry is a chemical division that evaluates the quantitative content of the chemical process with the help of the reacting molecules or products taking part in the reaction. The term “stoicheion” in “Stoichiometry”, is an old Greek term for "element" whereas “metron” means "measure".

Question

How many moles of NH3 can
be produced from 3.76 moles
of nitrogen in the following
reaction:
N2 (g) + 3 H2 (g) → 2 NH3 (g)
->

Expert Solution

This question has been solved!

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

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 2 steps with 2 images

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

An air bag is deployed by utilizing the following re tion the nitrogen gas produced inflates the air bag): :math>2NaN3(s)2Na(s)+3N2(g) 10.5 g of NaN1 is decomposed, what theoretical mass of sodium should be produced? If only 2.84 g of sodium is actually collected, what is the percent yield?
Air Pollution Nitrogen monoxide, which is present in urban air pollution, immediately Converts to nitrogen dioxide as it reacts with oxygen. a. Write the balanced chemical equation for the formation of nitrogen dioxide from nitrogen monoxide. b. What mole ratio would you use to convert from moles of nitrogen monoxide to moles of nitrogen dioxide?
It sodium peroxide is added to water, elemental oxygen gas is generated: :math>Na2O2(s)+H2O(l)NaOH(aq)+O2(g) ppose 3.25 g of sodium peroxide is added to a large excess of water. What mass of oxygen gas will be produced?
When potassium chlorate is subjected to high temperatures, it decomposes into potassium chloride and oxygen. (a) Write a balanced equation for the decomposition. (b) In this decomposition, the actual yield is 83.2%. If 198.5 g of oxygen are produced, how much potassium chlorate decomposed?
A power plant is driven by the combustion of a complex fossil fuel having the formula C11H7S. Assume the air supply is composed of only N2 and O2 with a molar ratio of 3.76:1.00, and the N2 remains unreacted. In addition to the water produced, the fuels C is completely combusted to CO2 and its sulfur content is converted to SO2. In order to evaluate gases emitted at the exhaust stacks for environmental regulation purposes, the nitrogen supplied with the air must also be included in the balanced reactions. a Including the N2 supplied m the air, write a balanced combustion equation for the complex fuel assuming 100% stoichiometric combustion (i.e., when there is no excess oxygen in the products and the only C-containing product is CO2). Except in the case of N2, use only integer coefficients. b Including N2 supplied in the air, write a balanced combustion equation for the complex fuel assuming 120% stoichiometric combustion (i.e., when excess oxygen is present in the products and the only C-containing product is CO2). Except in the case of use only integer coefficients c Calculate the minimum mass (in kg) of air required to completely combust 1700 kg of C11H7S. d Calculate the air/fuel mass ratio, assuming 100% stoichiometric combustion. e Calculate the air/fuel mass ratio, assuming 120% stoichiometric combustion.
Freon-12, CCl2F2, is prepared from CCl4 by reaction with HF. The other product of this reaction is HCl. Outline the steps needed to determine the percent yield of a reaction that produces 12.5 g of CCl2F2 from 32.9 g of Cd4. Freon-12 has been banned and is no longer used as a refrigerant because it catalyzes the decomposition of ozone and has a very long lifetime in the atmosphere. Determine the percent yield.
For each of the following balanced equations, indicate how many moles of the product could be produced by complete reaction of 1.00 g of the reactant indicated in boldface. Indicate clearly the mole ratio used for the conversion. msp;NH3(g)+HCl(g)NH4Cl(s) msp;CaO(s)+CO2(g)CaCO3(s) msp;4Na(s)+O2(g)2Na2O(s) msp;2P(s)+3Cl2(g)2PCl3(l)
4.19 How many metric tons of carbon are required to react with 7.83 metric tons of Fe2O3 according to the following reaction? 2Fe2O3+3C3CO2+4Fe How many metric tons of iron are produced?
Solid silicon dioxide, often called silica, reacts with hydrofluoric acid (HF) solution to produce the gas silicon tetrafluoride and water. a. Write the balanced chemical equation for the reaction. b. List three mole ratios, and explain how you would use them in stoichiometric calculations.
Titanium dioxide, TiO2 , reacts with carbon and chlorineto give gaseous TiCl4 : TiO2+2C+2Cl2TiCl4+2CO The reaction of 7.39 kg titanium dioxide with excess Cand Cl2 gives 14.24 kg titanium tetrachloride. Calculatethe theoretical yield of TiCl4 (assuming complete reaction)and its percentage yield.
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)
Solid calcium carbide (CaC2)reacts with liquid water to produce acetylene gas (C2H2)and aqueous calcium hydroxide. l type='a'> Write the balanced equation for the reaction that is (occurring. including all phases. If a 100.0-g sample of calcium carbide (CaC2)is initially reacted with 50.0 g of water, which reactant is limiting? Prove that mass is conserved for the reactant amounts used in pan b.