6. The reaction of ozone with methane produces carbon dioxide and water vapour. CH4(g)+ 4/3 Os(g)-...
Part ACalculate the bond energy per mole for breaking all the bonds in methane, CH4.Express your answer to four significant figures and include the appropriate units.ΔHCH4 =1656 kJmolCorrectIn CH4, the energy required to break one C−H bond is 414 kJ/mol. Since there are four C−H bonds in CH4, the energy ΔHCH4 for breaking all the bonds is calculated asΔHCH4=4×bond energy of C−H bond=4×414 kJ/mol=1656 kJ/mol CH4 moleculesPart BCalculate the bond energy per mole for breaking all the bonds of oxygen,...
QUESTION 4 Using bond-energy data, what is AHⓇ for the following reaction? CH4(g) + 2F2(g) - CF4(g) + 2H2(g) Bond Bond Energy (kJ/mol) C-H 413 432 159 Н-Н F-F C-F O a. 1489 kJ Ob.561 kJ O c. 834 kJ d. -561 kJ O e.-834 kJ
4. Glucose (CaHi2 is metabolized by a combustion reaction to form carbon dioxide and water. (glucose has 5 C-C, 7 C-O, 5 0-H, 7 CH) a) Write a balanced reaction C6 H,,06(s) +60,(リーウ.coz(S) t 6H20,9 н-о Determine the enthalpy for the reaction using the bond enthalpies listed in the table. Is the reaction endothermic or exothermic? b) Bond Enthalpy (kJ/mol) Bond C-C C-O O-H C-H O-O 347 351 460 414 498.7 799 c) How much glucose (in g) must be...
Methane, CH4, reacts with oxygen to produce carbon dioxide, water, and heat. CH49) + 2O2(g) - CO2(g) + 2H2O() What is the value of AH if 5.00 g of CH4 is combusted? 157 kJ 277 kJ 445 kJ -714 kJ 1.43 104 kJ
The combustion of methane (CH4) at 298.0 K produces carbon dioxide gas (CO2) and liquid water. A constant volume vessel of volume V = 0.807 L is loaded with 1.000 mole of each methane and oxygen. Find the total pressure in bar after the reaction has taken place at 298 K. Use an ICE box, and for now you may assume the reaction goes to completion at 298 K
The following thermochemical equation is for the reaction of methane(g) with oxygen(g) to form carbon dioxide(g) and water(g). CH4(g) + 2O2(g) ---> CO2(g) + 2H2O(g) H = -802 kJ When 6.37 grams of methane(g) react with excess oxygen(g), ___ kJ of energy are _________(evolved or absorbed). Once you get the answer, would it be a negative number or a positive number?
3. (3 pt) In the combustion of methane gas, CH4 (g), how many liters of carbon dioxide gas are generated from the complete combustion of 12.5 grams of methane in an excess of oxygen? (Assume the conditions after the reaction is completed are P-0.992 atm and T-27.3°C.) CO-H-O CHy
Now 3 The combustion of octane to form carbon dioxide and liquid water can be written as: CH3(g) +2502(g) → 8C02(g) +9H, O(1) AH = -5450kJ mol-1 The combustion of octane to form carbon dioxide and water vapour can be written as: C2H18(8)+ 25 02(g) → 8C02()+9H, O(g) How would the energy released by the combustion of 1 mol of octane to form water vapour compare with the energy released by 1 mol of octane to form liquid water? 5
Use the bond energies below to estimate AH for the following reaction: CH4 (g) + Cl2 (g) - CH3CI (g) + HCl (g) Bond Energies (kJ/mole) single bonds. multiple bonds H C. Cl H. 432. C=O 799 C. 412. 346. C=C.602 O. 459. 358. 142 C=C 835 Cl 431. 328. 242. O=O 494
PART ONE: PART TWO: PART THREE: PART FOUR: Gaseous methane (CH4) will react with gaseous oxygen (O2) to produce gaseous carbon dioxide (CO2 and gaseous water (H20). Suppose 13. g of methane is mixed with 13.8 g of oxygen. Calculate the minimum mass of methane that could be left over by the chemical reaction. Round your answer to 2 significant digits A 1.32-g sample of a compound is burned in a bomb calorimeter, producing a temperature change from 20.85 °C...