Under certain circumstances, carbon dioxide,CO2 (g), can be made to react with hydrogen gas,H2 (g), to produce methane, CH (g), and watervapor, H20(g):Part ACO2(g) + 4H2 (g)→CH4(g) + 2H2O(g)How many moles of methane are produced when 36.6 moles of carbon dioxide gas react with excess hydrogen gas?Express your answer with the appropriate units.• View Available Hint(s)HÀValueUnits

Since from the above given balanced reaction, 1 mole of CO2 is reacting to form 1 mole of methane…

Answered: Under certain circumstances, carbon…

World of Chemistry

7th Edition

ISBN:9780618562763

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter9: Chemical Quantities

Section: Chapter Questions

Problem 55A

See similar textbooks

Similar questions

Hydrogen cyanide, HCN, can be made by a two-step process. First, ammonia is reacted with O2 to give nitric oxide, NO. 4NH3(g)+5O2(g)4NO(g)+6H2O(g) Then nitric oxide is reacted with methane, CH4. 2NO(g)+2CH4(g)2HCN(g)+2H2O(g)+H2(g) When 24.2 g of ammonia and 25.1 g of methane are used, how many grams of hydrogen cyanide can be produced?
Write the balanced chemical equation for the complete combustion of heptene, C7H14. In combustion, hcpLcnc reacts with oxygen to produce carbon dioxide and water. What is the mole ratio that would enable you to calculate the number of moles of oxygen needed to react exactly with a given number of moles of heptene? What mole ratios would you use to calculate how many moles of each product form from a given number of moles of heptene?
Propane, C3H8, is the fuel of choice in a gas barbecue. When burning, the balanced equation is C3H8+5O23CO2+4H2O a What is the limiting reactant in cooking with a gas grill? b If the grill will not light and you know that you have an ample flow of propane to the burner, what is the limiting reactant? c When using a gas grill you can sometimes turn the gas up to the point at which the flame becomes yellow and smokey. In terms of the chemical reaction, what is happening?
You react nitrogen and hydrogen in a container to produce ammonia, NH3(g). The following figure depicts the contents of the container after the reaction is complete. a Write a balanced chemical equation for the reaction. b What is the limiting reactant? c How many molecules of the limiting reactant would you need to add to the container in order to have a complete reaction (convert all reactants to products)?
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)
The principal constituent of natural gas is methane, which burns in air according to the reaction CH4+2O2CO2+2H2O How many grams of O2 are needed to produce 3.50 g of CO2?
Ammonia can be formed by a direct reaction of nitrogen and hydrogen. N2(g) + 3 H2(g) 2 NH3(g) A tiny portion of the starting mixture is represented by the diagram, where the blue circles represent N and the white circles represent H. Which of these represents the product mixture? For the reaction of the given sample, which of these statements is true? (a) N2 is the limiting reactant. (b) H2 is the limiting reactant. (c) NH, is the limiting reactant. (d) No reactant is limiting: they are present in the correct stoichiometric ratio.
Under certain circumstances, carbon dioxide, CO2(g)CO2(g), can be made to react with hydrogen gas, H2(g)H2(g), to produce methane, CH4(g)CH4(g), and water vapor, H2O(g)H2O(g): CO2(g)+4H2(g)→CH4(g)+2H2O(g) A.How many moles of methane are produced when 85.1 molesmoles of carbon dioxide gas react with excess hydrogen gas? Express your answer with the appropriate units. B. How many moles of hydrogen gas would be needed to react with excess carbon dioxide to produce 76.6 molesmoles of water vapor? Express your answer with the appropriate units.
17. Under certain circumstances, carbon dioxide, CO2(g)CO2(g), can be made to react with hydrogen gas, H2(g)H2(g), to produce methane, CH4(g)CH4(g), and water vapor, H2O(g)H2O(g): CO2(g)+4H2(g)→CH4(g)+2H2O(g) A. How many moles of methane are produced when 85.1 molesmoles of carbon dioxide gas react with excess hydrogen gas? Express your answer with the appropriate units. B. How many moles of hydrogen gas would be needed to react with excess carbon dioxide to produce 76.6 molesmoles of water vapor? Express your answer with the appropriate units.
Under certain circumstances, carbon dioxide, CO2(g), can be made to react with hydrogen gas, H2(g), to produce methane, CH4(g), and water vapor, H2O(g): CO2(g)+4H2 (g)→CH4(g)+2H2O(g) How many moles of methane are produced when 25.1 moles of carbon dioxide gas reacts with excess hydrogen gas? Express your answer with the appropriate units.
queous hydrobromic acid HBr reacts with solid sodium hydroxide NaOH to produce aqueous sodium bromide NaBr and liquid water H2O . What is the theoretical yield of water formed from the reaction of 3.2g of hydrobromic acid and 2.8g of sodium hydroxide?Be sure your answer has the correct number of significant digits in it.
Under certain circumstances, carbon dioxide, CO2(g)CO2(g), can be made to react with hydrogen gas, H2(g)H2(g), to produce methane, CH4(g)CH4(g), and water vapor, H2O(g)H2O(g): CO2(g)+4H2(g)→CH4(g)+2H2O(g) How many moles of methane are produced when 25.1 molesmoles of carbon dioxide gas react with excess hydrogen gas? Express your answer with the appropriate units. For example, write the unit moles as mol. How many moles of hydrogen gas would be needed to react with excess carbon dioxide to produce 88.1 molesmoles of water vapor? Express your answer with the appropriate units. For example, write the unit moles as mol.

SEE MORE QUESTIONS

Recommended textbooks for you

World of Chemistry

Chemistry

ISBN:

9780618562763

Author:

Steven S. Zumdahl

Publisher:

Houghton Mifflin College Div

Introductory Chemistry: A Foundation

Chemistry

ISBN:

9781337399425

Author:

Steven S. Zumdahl, Donald J. DeCoste

Publisher:

Cengage Learning

Chemistry for Engineering Students

Chemistry

ISBN:

9781337398909

Author:

Lawrence S. Brown, Tom Holme

Publisher:

Cengage Learning

World of Chemistry

Chemistry

ISBN:

9780618562763

Author:

Steven S. Zumdahl

Publisher:

Houghton Mifflin College Div

Introductory Chemistry: A Foundation

Chemistry

ISBN:

9781337399425

Author:

Steven S. Zumdahl, Donald J. DeCoste

Publisher:

Cengage Learning

Chemistry for Engineering Students

Chemistry

ISBN:

9781337398909

Author:

Lawrence S. Brown, Tom Holme

Publisher:

Cengage Learning

Living By Chemistry: First Edition Textbook

Chemistry

ISBN:

9781559539418

Author:

Angelica Stacy

Publisher:

MAC HIGHER

General, Organic, and Biological Chemistry

Chemistry

ISBN:

9781285853918

Author:

H. Stephen Stoker

Publisher:

Cengage Learning

General Chemistry - Standalone book (MindTap Cour…

Chemistry

ISBN:

9781305580343

Author:

Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell

Publisher:

Cengage Learning

SEE MORE TEXTBOOKS