How does the heat produced when 1 mole ofC is burned directly to CO2by the reactionC(s) + O2(g)→CO2(g)compare with that produced when 1 mole ofC undergoes the two-step process:C(s) +12O2(g)→CO(g) morrison (gjm2355) – Chapter 17 – andrews – (7)2CO(g) +12O2(g)→CO2(g)if all reactants and products are at the same temperature and pressure? 1.The heat produced is the same either way. 2.More heat is produced in the two-step process. 3.Cannot tell without calculating the heat produced. 4.More heat is produced in the one-step process.

How does the heat produced when 1 mole ofC is burned directly to CO2by the reactionC(s) + O2(g)→CO2(g)compare with that produced when 1 mole ofC undergoes the two-step process:C(s) +12O2(g)→CO(g) morrison (gjm2355) – Chapter 17 – andrews – (7)2CO(g) +12O2(g)→CO2(g)if all reactants and products are at the same temperature and pressure? 1.The heat produced is the same either way. 2.More heat is produced in the two-step process. 3.Cannot tell without calculating the heat produced. 4.More heat is produced in the one-step process.

Introductory Chemistry: A Foundation

8th Edition

ISBN:9781285199030

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter10: Energy

Section: Chapter Questions

Problem 66AP: Calculate the enthalpy change when 1.0(1 g of methane is burned in excess oxygen according to the...

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Given the following reactions Fe2O3 (s) + 3CO (s) → 2Fe (s) + 3CO2 (g) ΔH = -26.6 kJ 3Fe (s) + 4CO2 (s) → 4CO (g) + Fe3O4 (s) ΔH = +10.2 kJ the enthalpy of the reaction of Fe2O3 with CO 3Fe2O3 (s) + CO (g) → CO2 (g) + 2Fe3O4 (s) is __________ kJ.
The same student wanted to determine the heat of dissolution for potassium chlorate (KClO3, MW: 122.55 g/mol) in water. He measured 10 grams of KClO3 and dissolved it in a calorimeter containing 250 g of water. The temperature drop was 3.5 K. 1. What is qH2O in Joules? A. +146.4 B. -146.4 C. -3661 D. +3661 2. What is qdissolution in Joules? A. +146.4 B. -146.4 C. -3661 D. +3661 3. What is the ΔHdissolution in kilojoules per mole? A. +44.866 B. -44.866 C. +1.794 D. -1.794 4. Is the reaction endothermic or exothermic? A. Endothermic B. Exothermic
It is interesting to compare the “fuel value” of a hydrocarbonin a hypothetical world where oxygen is not thecombustion agent. The enthalpy of formation of CF41g2 is-679.9 kJ>mol. Which of the following two reactions is themore exothermic?CH41g2 + 2 O21g2 ¡ CO21g2 + 2 H2O1g2CH41g2 + 4 F21g2 ¡ CF41g2 + 4 HF1g2
To a test tube containing 5.0 ml of 1.00 M NaOH at 27°C in a calorimeter, 5.0 ml of 2.00 M HNO3 at the same temperature was added, the heat generated by the reaction was monitored. Which of the following is TRUE? a.Reaction is exothermic; solution will turn pink upon addition of phenolphthalein. b.Heat is absorbed by the system; no color change will be observed upon addition of phenolphthalein. c.Heat is released by the system; no color change will be observed upon addition of phenolphthalein. d.Reaction is endothermic; solution will turn pink upon addition of phenolphthalein.
What is the enthalpy change when 175 g of C3H8 are burned in excess O2?C3H8(g) + 5 O2(g)  3 CO2(g) + 4 H2O(l) H = -2220 kJa. -1.71  107 kJb. -1.79  10-3 kJc. -3.47  100 kJd. -3.89  105 kJe. -8.83  103 kJ
When 0.2490 moles of methane, CH4(g) is burned in excess oxygen at thermodynamic standard state, 221.74 kJ of heat is released. What is ΔHfor the combustion for 1 mole of methane, CH4(g)? CH4(g) + 2 O2(g) -> CO2(g) + 2 H2O(l) ΔHrxn= ______________________ 2) What is the enthalpy change for making exactly 2 moles of methane (instead of combusting the methane) by the following reaction: CO2(g) + 2 H2O(l) -> CH4(g) + 2 O2(g)
When 0.2490 moles of methane, CH4(g) is burned in excess oxygen at thermodynamic standard state, 221.74 kJ of heat is released. What is ΔH for the combustion for 1 mole of methane,CH4(g)? CH4(g) + 2 O2(g) à CO2(g) + 2 H2O(l)
Ethylene (C₂H₄) is the starting material for the preparationof polyethylene. Although typically made during the processingof petroleum, ethylene occurs naturally as a fruit-ripening hor-mone and as a component of natural gas. (a) The heat of reactionfor the combustion of C₂H₄ is 1411 kJ/mol. Write a balancedthermochemical equation for the combustion of C₂H₄. (b) Howmany grams of C₂H₄ must burn to give 70.0 kJ of heat?
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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.
how much heat be given off when 18.5g of c2h4 is burned in oxygen to form CO2g