Concept explainers
Interpretation:
The given reaction has to be identified that it belongs to exothermic or endothermic.
Concept Introduction:
Energy: It is the capacity or ability to do work. Joule (J) is the SI unit of energy.
Enthalpy H is the amount energy absorbed or released in a process.
Where,
Exothermic reaction: Exothermic reactions are those in which evolution of heat takes place during chemical reaction.
Endothermic reaction: Endothermic reactions are
Want to see the full answer?
Check out a sample textbook solutionChapter 4 Solutions
OWLv2 for Moore/Stanitski's Chemistry: The Molecular Science, 5th Edition, [Instant Access], 1 term (6 months)
- Use the appropriate tables to calculate H for (a) the reaction between copper(II) oxide and carbon monoxide to give copper metal and carbon dioxide. (b) the decomposition of one mole of methyl alcohol (CH3OH) to methane and oxygen gases.arrow_forwardCalcium carbide, CaC2, is manufactured by reducing lime with carbon at high temperature. (The carbide is used in turn to make acetylene, an industrially important organic chemical.) Is the reaction endothermic or exothermic?arrow_forward4.60 Why are fuel additives used?arrow_forward
- Which molecule, F2, Cl2, Br2, or I2, has the weakest chemical bond?arrow_forwardThe equation for the fermentation of glucose to alcohol and carbon dioxide is: C6H12O6(aq) 2C2H5OH(aq) + 2CO2(g) The enthalpy change for the reaction is 67 kJ. Is this reaction exothermic or endothermic? Is energy, in the form of heat, absorbed or evolved as the reaction occurs?arrow_forwardWhen lightning strikes, the energy can force atmospheric nitrogen and oxygen to react to make NO: N2(g)+O2(g)2NO(g)H=+181.8kJ (a) Is this reaction endothermic or exothermic? (b) What quantities of reactants and products are assumed if H = +181.8 kJ? (c) What is the enthalpy change when 3.50 g nitrogen is reacted with excess O2(g)?arrow_forward
- What is incomplete combustion of fossil fuels? Why can this be a problem?arrow_forwardA rebreathing gas mask contains potassium superoxide, KO2, which reacts with moisture in the breath to give oxygen. 4KO2(s)+2H2O(l)4KOH(s)+3O2(g) Estimate the grams of potassium superoxide required to supply a persons oxygen needs for one hour. Assume a person requires 1.00 102 kcal of energy for this time period. Further assume that this energy can be equated to the heat of combustion of a quantity of glucose, C6H12O6, to CO2(g) and H2O(l). From the amount of glucose required to give 1.00 102 kcal of heat, calculate the amount of oxygen consumed and hence the amount of KO2 required. The ff0 for glucose(s) is 1273 kJ/mol.arrow_forwardCH, (g) 20, (g) → CO, (g) + 2 H,O (g) + Exothermic or endothermicarrow_forward
- Fe2O3(s) + 3CO(s) → 2Fe(s) + 3CO2(g) ΔH = -28.0 kJ 3Fe(s) + 4CO2(s) → Fe3O4(s) + 4CO(g) ΔH = +12.5 kJ The enthalpy of reaction of Fe2O3 with CO 3Fe2O3(s) + CO(g) → CO2(g) + 2Fe3O4(s) is ____kJ.arrow_forwardUse the indicated average bond enthalpies to estimate the change in enthalpy, ΔHo, for the reaction between methane and iodine to produce iodomethane and hydrogen iodide: CH4(g) + I2(g) → CH3I(g) + HI(g) ΔHo = ? It may be helpful to draw the Lewis electron dot structure for each reactant and product; all reactants and products have single bonds. average bond enthalpies (kJ) C - H 413 , C - I 240 , H - I 299 , I - I 151 Express your answer in units of kilojoules, but do not include the units on your submitted answer.arrow_forwardWhat is the enthalpy of the reaction P406 (s) + 202(g)→P4010(s), given a) P4(s) + 302(g)→P406 AH = -1640.1 kJ/mol b) 2P4(s) + 1002(g)→2P4O10(s), AH = -5880.2 kJ/molarrow_forward
- Chemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage LearningChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage LearningChemistry: An Atoms First ApproachChemistryISBN:9781305079243Author:Steven S. Zumdahl, Susan A. ZumdahlPublisher:Cengage Learning
- World of Chemistry, 3rd editionChemistryISBN:9781133109655Author:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCostePublisher:Brooks / Cole / Cengage LearningChemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage Learning