15. Methane gas (CH4) reacts with oxygen gas (O2) according to theequation below. This reaction releases 890kJ of energy for each mole ofmethane gas that is consumed. Which of the following BEST describes thisreaction? *CH4+ 202 → CO2 + 2H2O + energyA. The reaction is endothermic; CO2 and H20 have more chemical potential energythan CH4 and 02.B. The reaction is endothermic; CO2 and H20 have less chemical potential energythan CH4 and 02.C. The reaction is exothermic; CO2 and H20 have more chemical potential energythan CH4 and 02.D. The reaction is exothermic; CO2 and H20 have less chemical potential energy thanCH4 and 02.

CH4 + 2O2----> CO2 + 2H2O + energy

5. Methane gas (CH4) reacts with oxygen gas (02) according to the quation below. This reaction releases 890kJ of energy for each mole nethane gas that is consumed. Which of the following BEST describes eaction? * CH4+ 202 > CO2 + 2H,0 + energ A. The reaction is endothermic; CO2 and H20 have more chemical potential er than CH4 and 02. B. The reaction is endothermic; CO2 and H20 have less chemical potential ene- than CH4 and 02. C. The reaction is exothermic; CO2 and H20 have more chemical potential ener than CH4 and 02.

5. Methane gas (CH4) reacts with oxygen gas (02) according to the quation below. This reaction releases 890kJ of energy for each mole nethane gas that is consumed. Which of the following BEST describes eaction? * CH4+ 202 > CO2 + 2H,0 + energ A. The reaction is endothermic; CO2 and H20 have more chemical potential er than CH4 and 02. B. The reaction is endothermic; CO2 and H20 have less chemical potential ene- than CH4 and 02. C. The reaction is exothermic; CO2 and H20 have more chemical potential ener than CH4 and 02.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

[Review Topics] The overall reaction in commercial heat packs can be represented as 4Fe(8) + 30₂(g) → 2Fe2O3 (8) AH = -1652 kJ a. How much heat is released when 4.44 mol iron is reacted with excess O2? kJ released b. How much heat is released when 1.58 mol Fe2O3 is produced? kl released c. How much heat is released when 1.73 g iron is reacted with excess O2? kJ released d. How much heat is released when 11.1 g Fe and 2.75 g O2 are reacted? Submit Answer kJ released Retry Entire Group [References] 9 more group attempts remaining Previous
Part of the industrial recovery of elemental zinc from the zinc sulfide ore is by roasting: ZnS) + O2(2) → ZnOs + SO22) AH = -879 kJ/mol Calculate the amount of heat (in kJ) released when 1.00 g of zinc sulfide reacts with excess oxygen.
None
Calculate the standard enthalpy of reaction for: C2H2 ---> 2 C + H2 If, 2 C2H2 + 5 O2 ----> 4 CO2 + 2 H2O (Standard Enthalpy = -2600 kJ/mole) C + O2 ---> CO2 (Standard Enthalpy = -390 kJ/mole) 2 H2 + O2 ---> 2 H2O (Standard Enthalpy = -590 kJ/mole)
How much energy in kJ is required to decompose 765 g of PCI3, according to the reaction below? (PCI3:137.32 g/mol) 31 - 4 PC13(g) → P4(s) + 6 Cl2(g) AH°rxn =+1207 kJ O A) 1681 O B) 7016 O C) 5950 O D) 4582 O E) 2310
7. Which of the following technologies are considered non-renewable energy sources? Choose ALL that apply. a. Coal Power Plants b. C. Hydrogen Fuel Cells Fossil Fuel Power Plants a. b. C. 8. Which of the following reactions are endothermic? Choose ALL that apply. H2(g) + 1/2O2(g) H₂O(g); AH = -243 kJ/mol ¹1/2N2(g) + ¹//202(g) + 90.7 kJ → NO(g) CO(g) + 111 kJ C(s) + ¹1/202(g) d. Hydroelectric Generators Solar Panels e. f. Wind Turbines a. Acid lonization Constant (K₂) b. Base lonization Constant (K) C. Equilibrium Constant (Keg) d. e. f. HI(g)→→ ¹1/₂2H2(g) + ½l2(g); AH = −26 kJ/mol H₂O(g) · H2(g) + ½O2(g); AH = +243 kJ/mol + O2(g) 2NO N2(g) + 181.4 kJ (g) 9. Which equilibrium constant would be most relevant to the following system in equilibrium: HC₂H3O2(aq) → H*( (aq) + C₂H3O₂ (aq) Partial Pressure Equilibrium Constant (K₁) d. e. Solubility Product Constant (Ksp) f. Water lon Product Constant (Kw)
Consider the reaction below with the indicated heats of formation. 2 N2O (g) + O2 (g) --> 4 NO (g) +82 kJ/mol +90 kJ/mol What is the energy absorbed or released when 1.0 mol of NO is produced? a. -196 kJ b. +23 kJ c. +49 kJ d. +90 kJ e. +196 kJ f. we cannot calculate the answer without knowing the heat of formation of oxygen gas
The value of AH° for the reaction below is -126 kJ. The amount of heat that is released by the reaction of 10.0 g of Na 20 2 with water is kJ. 2Na 20 2 (s) + 2H 20 (I) → 4NaOH (s) + O 2 (g) A 16.2 В 67.5 32.3 -126 E 8.08
Calculate AH for the reaction of sulfur dioxide with oxygen. 2SO2 (g) + O2 (g) –→ 2SO3 (g) (AHf ° SO2 (g) = -296.8 kJ/mol; AHf ° SO3 (g) = -395.7 kJ/mol) Select one: O a. -98.9 kJ O b. -197.8 kJ O c. Not enough information is given. O d. 197.8 kJ
I need help answering 4c.
How many g Al must react with iodine to form AlI₃ via the following reaction scheme to release -836.0 kJ of heat? 2 Al(s) + 3 I₂(s) → 2 AlI₃(s) ∆H = -302.9 kJ
Con‎sider follo‎wing reaction: ‎ (s) -> Hg(l) + ½ O2 (g) DH = +90.7 kj/mol. Which of the following statements is false ? a. The‎ formati‎on of HgO (s) fr‎om liquid H‎g and gase‎ous O2 will relea‎se heat. b. T‎he rea‎ction will oc‎cur at all temp‎eratures. c. The f‎orward rea‎ction is endot‎hermic. Giv‎en following reaction 2 Fp‎2(g) + O2(g) --> 2F2O (g) Delta H= -43.4 kJ Delt‎a S (Ent‎ropy) for the rea‎ction is < 0 because a.Del‎ta H is ne‎gative b. The‎re is less‎ disorder wh‎en prod‎ucts are form‎ed as there are les‎s mole‎s in produ‎ct side compare‎d to reactant side c. Rxn is ex‎othermic, exoth‎ermic reactio‎ns are always‎ spont‎aneous Spo‎ntaneity of re‎action can be deter‎mined by a. En‎tropy b. W‎ork; c. H‎eat of Enthal‎py d. Gib‎bs Fre‎e Ene‎rgy