
Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
expand_more
expand_more
format_list_bulleted
Question
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.
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
Trending nowThis is a popular solution!
Step by stepSolved in 2 steps

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
- Excess sodium bicarbonate (NaHCO3) is added to a 250. mL solution sulfuric acid (H2SO4). The sodium bicarbonate the sulfuric acid react as shown below, producing liquid water, carbon dioxide gas and aqueous sodium sulfate. 1 H2SO4 (aq) + 2 NaHCO3 (s) → 2 H20 (I) + 2 CO2 (g) +1 NazSO4(aq) The temperature is 29.°C, and the volume of gas produced, collected in an inverted cylinder over water, is 175. mL. Assume this reaction goes to completion. If the total pressure inside the inverted cylinder at the end of the reaction is 316 torr, what was the molarity of the sulfuric acid solution?arrow_forwardEthanol (C2H5OH) and oxygen gas (O2) react to form carbon dioxide (CO2) and water (H20): C2H5OH(1) + 302(g) → 2CO2(g) + 3H20(g) What can be concluded from the chemical equation?arrow_forwardThe complete combustion of gasoline (C8H18) is best represented by which of the following equations: 2 C8H18 (l) + 25 O2 (g) → 16 CO2 (g) + 18 H2O(l) 2 C8H18 (l) + 17 O2 (g) → 16 CO (g) + 9 H2O (l) C8H18 (l) → 8 C (s) + 9 H2 (g) C8H18 (l) + O2(g) → 8 CO2 (g) + 9 H2O (l) C8H18 (l) + O(g) → 8 CO2 (g) + 9 H2O (l)arrow_forward
- 2NO(g) + O2(g) → 2NO2(g) You are provided with 4.12 molmol of nitrogen monoxide gas. Using the balanced chemical equation completed in Part A, determine how many moles of oxygen gas are needed to completely react with the nitrogen monoxide gas and how many moles of nitrogen dioxide are formed as a result? Ammonia and oxygen react to form nitrogen monoxide and water. Construct your own balanced equation to determine the amount of NO and H2O that would form when 2.80 molmol NH3 and 4.64 mol O2 react. Express the amounts in moles to two decimal places separated by a comma.arrow_forwardFor the following chemical reaction, N2 (g) + 3 H2 (g) → 2 NH3 (g) If 15 molecules of nitrogen gas and 12 molecules of hydrogen gas react together what will be left in the container at the end of the reaction.arrow_forwardWhat is the easiest process to get to the result?arrow_forward
- The extraction of aluminum metal from the aluminum hydroxide found in bauxite by the Hall-Héroult process is one of the most remarkable success stories of 19th century chemistry, turning aluminum from a rare and precious metal into the cheap commodity it is today. In the first step, aluminum hydroxide reacts to form alumina Al2O3 and water: 2Al(OH)3(s) + Al2O3(s) -> 3H2O(g) In the second step, alumina Al2O3 and carbon react to form aluminum and carbon dioxide: 2Al2O3(s) + 3C(s) + 4Al(s) -> 3CO2(g) Suppose the yield of the first step is 74.% and the yield of the second step is 76.% . Calculate the mass of aluminum hydroxide required to make 4.0kg of aluminum. Be sure your answer has a unit symbol, if needed, and is rounded to the correct number of significant digits.arrow_forwardDimethyl ether, a useful organic solvent, is prepared in two steps. In the first step, carbon dioxide and hydrogen react to form methanol and water: CO₂(g) + 3 H₂(g) CH₂OH(1) + H₂O(1) In the second step, methanol reacts to form dimethyl ether and water: 2 CH₂OH(1)→ CH₂OCH3(g) + H₂O(1) Calculate the net change in enthalpy for the formation of one mole of dimethyl ether from carbon dioxide and hydrogen from these reactions. Round your answer to the nearest kJ. เม kJ AH=-131. kJ Ś ΔΗ= 8. kJarrow_forwardThe human body burns glucose (C6H₁2O6) for energy according to this chemical reaction: C6H12O6 +60₂-6CO₂ + 6H₂O The products of the reaction are carbon dioxide (CO₂) and water (H₂O). Interestingly, all of the carbon dioxide and much of the water exits the body through the lungs: on every breath, the average person exhales 500. mL of air, which is typically enriched to 4% CO₂ and 5% water vapor by volume. In short, when a person loses weight by dieting, the weight that is lost actually departs his body as a gas, every time he exhales. Each kilogram of body fat lost requires exhaling about 2.9 kg of carbon dioxide. Calculate how many breaths it takes an average person to "exhale" 1.00 kg of fat. Round your answer to the nearest thousand. You'll need to know that the density of CO₂ is 2.0 kg/m³. 0 ☐ ☐x10 Xarrow_forward
- Consider the following balanced equation. 3 Ag(s) + 4 HNO3(aq) → 3 AgNO3(aq) + NO(g) + 2 H2O(l) A student used 117.24 g of Ag and obtained 135.49 g of AgNO3, calculate the percent yield of AgNO3. Give your answer to the correct number of significant figures without unit. Molar mass of Ag: 107.87 g/mol Molar mass of HNO3: 63.01 g/mol Molar mass of AgNO3: 169.87 g/mol Molar mass of NO: 30.01 g/mol Molar mass of H2O: 18.02 g/molarrow_forwardNitric acid is often manufactured from the atmospheric gases nitrogen and oxygen, and hydrogen prepared by reforming natural gas, in a two-step process. In the first step, nitrogen and hydrogen react to form ammonia: N₂(g) + 3H₂(g) 2 NH, (g) In the second step, ammonia and oxygen react to form nitric acid (HNO3) and water: NH₂ (g) + 20₂(g) → HNO3(g) + H₂O (g) Suppose the yield of the first step is 61.% and the yield of the second step is 77.%. Calculate the mass of nitrogen required to make 10.0 kg of nitric acid. Be sure your answer has a unit symbol, if needed, and is rounded to 2 significant digits. 0 Explanation Check. ☐ x10 8 X 09 0.0 S © 2023 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center |arrow_forwardIn one sentence explain what's wrong with this equation, and rewrite it so that the coefficients are correct. C3H6(g)+4.5 O2(g)->3CO2(g)+3H2O(g)arrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
- ChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage LearningChemistryChemistryISBN:9781259911156Author:Raymond Chang Dr., Jason Overby ProfessorPublisher:McGraw-Hill EducationPrinciples of Instrumental AnalysisChemistryISBN:9781305577213Author:Douglas A. Skoog, F. James Holler, Stanley R. CrouchPublisher:Cengage Learning
- Organic ChemistryChemistryISBN:9780078021558Author:Janice Gorzynski Smith Dr.Publisher:McGraw-Hill EducationChemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage LearningElementary Principles of Chemical Processes, Bind...ChemistryISBN:9781118431221Author:Richard M. Felder, Ronald W. Rousseau, Lisa G. BullardPublisher:WILEY

Chemistry
Chemistry
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning

Chemistry
Chemistry
ISBN:9781259911156
Author:Raymond Chang Dr., Jason Overby Professor
Publisher:McGraw-Hill Education

Principles of Instrumental Analysis
Chemistry
ISBN:9781305577213
Author:Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:Cengage Learning

Organic Chemistry
Chemistry
ISBN:9780078021558
Author:Janice Gorzynski Smith Dr.
Publisher:McGraw-Hill Education

Chemistry: Principles and Reactions
Chemistry
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:Cengage Learning

Elementary Principles of Chemical Processes, Bind...
Chemistry
ISBN:9781118431221
Author:Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:WILEY