8.66 ) Question 4 (1 point) Using bond energies, calculate the heat of combustion of ethylene,...
QUESTION 1 Calculate the heat of reaction (energy of reaction) in kJ/mol for the following reaction. Mind the correct sign of your answer value! 2 CO(g) + O2(g) →→2C02(g) Use the following bond energies for your calculation. Bond energies (kJ/mol) Bond Energy Bond Energy H-H 436 (-O 336 C-H 416 C=C 598 N–H 391 050 498 0-H 467 (=O 803 c-c 356 N=N 946 146 CEO 1073 LO
QUESTION 2 Calculate the heat of reaction (energy of reaction) in kJ/mol for the following reaction. Mind the correct sign of your answer value! 2C2H6(g) + 702(g) —+ 4CO2(g) + 6H2O(g) Use the following bond energies for your calculation. UŻ OU Bond energies (kJ/mol) Bond Energy Bond Energy H-H 436 (-O 336 (-H 416 C=C 598 N-H 391 O=0 498 467 C=0 803 c-c 356 N=N 946 0-0 146 CEO 1073
Question 4 1 pts Use the given average bond energies to calculate AHrxn for the following chemical reaction. Н н 20 c= o 3 0 O + зн—о—Н C Н Н Bond Bond energy (kJ/mol) C-O 360 C O 707 O O 498 464 Н-о C-H 414 +242 kJ O +914 kJ -914 kJ -242 kJ -2106 kJ
c.) Using the table and your complete Lewis structures of glucose, ethanol and carbon dioxide, calculate the total energy in kJ/mol required to break the bonds in one mole of each of the three compounds. Show all calculations and appropriate units. Then determine if the reaction is exothermic or endothermic. reaction: C6H1206 -> 2 C2H5OH + 2 CO2 Table 4.4 Covalent Bond Energies (in kJ/mol) H C N O S F CI Br Single Bonds H 436 O ZOI 416...
Calculate the AH for the reaction below. CyHag) +30218) + CO2(g) + 2 H2O(1) The following are skeletal structures - lone pairs are not included H2 - CH2 + 3 0-020-C-O + 2H-O-H You can use the bond energy table below. Bond C-C C=C Cc H-C H-O 0-0 0-0 C=0 C=O (in CO,) Energy (kJ/mol 356 598 813 416 467 146 498 695 799 Show your work and submit a picture.
Question 2 4 pts Use the given average bond dissociation energies (BDE) to estimate A Hreaction for the combustion of hydrogen in oxygen that produces water: 2H2 (8) + O26 --> 2H20 (6) Bond BDE(kJ/mol) H-H 436 0-0 498 H-O 460
Name: Quiz 9 CHE 1030 1. Using the following bond energies Bond Energy (kJ/mol) 839 413 495 799 467 Bond C-H O-0 C-O O-H estimate the heat of combustion for 1 mol of acetylene: C2H2(g)+ O2(g) → 2CO2(g)+H2O(g) 2. Using the following data reactions: H2(g) + Cl2(g) → 2HCl(g) H2(g) → 2H(g) Cl2(g) 2CIg) AP (kJ) -184 432 239 calculate the energy of an H-Cl bond.
Question 6 0.5 pts The table below contains the bond dissociation energies for common bonds. 410 Dissociation energy Bond (kJ/mol) |C-c 350 CNC 611 C-H 350 (c=0 799 0-0 180 O=O 498 460 C-O H-o Calculate the bond dissociation energy required for breaking all the bonds in a mole of water molecules, H20. Express your answer numerically, in terms of kJ/mol, and to three significant figures.
Calculate the enthalpy for the reaction below using the following bond dissociation energies. • H-H 436 kJ/mol O-H 460 kJ/mol 0-0 180 kJ/mol • 0=0 498 kJ/mol H -774 kJ/mol -654 kJ/mol 654 kJ/mol 774 kJ/mol
the enthalpy change in a chemical reaction can be determined using bond energies. energy must be added or absorbed to break bonds and that energy is released when bonds are formed. therefore ,you can calculate the total enthalpy of the reaction using following formula: dH= bonds broken-bonds formed Using bond energies, calculate the change in energy that accompanies the following reaction: H2 + O2 -> 2H2O Bond Bond Energy H-H 432 kJ/mol O-O 498 kJ/mol H-O 467 kJ/mol