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6. Using the bond energy information provided below, calculate the AHreaction for the following chemical change....
please do not answer Using the bond energies provided below, calculate DH° for the reaction CH4(g) + 4C12(8) --> CC14(g) + 4HCI(g) Show calculation set-up. Bond: C-H CI-CI C-ci HCI Bond energy (kJ/mol): 413 243 339 427 O-110 kJ E) 440 kJ - 440 kJ 1422 k) O 110 kJ
a. b. For b is this table below: Bond Bond Energy, D (kJ/mol) C=0 1072 C1-C1 242 C-CI 339 C=0 732 Using the values of bond energy from the table above, estimate the enthalpy change for the following reaction: CO(g) + Cl2(9)—>COC12(E) DkJ Using average bond enthalpies (linked above), estimate the enthalpy change for the following reaction: H2(g) + 12(8)—2HI(g) kJ Submit Answer Retry Entire Group 6 more group attempts remaining Single Bonds H C N O F Si P...
1. a. Use the bond energy data provided to calculate AH.. for the following reaction. H-H + Cl-Cl → 2 H-CI Bond Bond Energy H-H 436 kJ/mol Cl-CI 243 kJ/mol H-CI 431 kJ/mol b. Based on your answer to part a, is the reaction an exothermic reaction or an endothermic reaction? Provide a brief explanation to support you choice of answer. An endothermic reaction occurs in a cylinder with initial volume of 1 L. 5 kJ of heat is transferred...
show work 9) Given the bond enthalpies Cl-Cl (243), C-CI (339), H-CI (431),C-H (414)all in kJ/mol, estimate AE for the following reaction: CH4(g)+ Cl2(g)-CH3Cl(g)+ HCl(g) A)-1427 k) B) -113 kJ C) -30 kJ D)-356 kJ E) 301 kJ
Use the bond energies given below to calculate the enthalpy change for the reaction, HCN(g) + 2 H2(g) → CH3NH2(g) Bond Bond Energy (kJ/mol) Bond Bond Energy (kJ/mol) H-H 432 C-H 413 C-N 305 C=N 615 C:N 891 N-H 391
The enthalpy change for the following reaction is 95.4 kJ. Using bond energies, estimate the N-H bond energy in N2H4(g). N2(g) + 2H2(g) N2H4(g) kJ/mol The enthalpy change for the following reaction is -92.2 kJ. Using bond energies, estimate the H-H bond energy in H2(g). 2NH3(g) N2(g) + 3H2(g) kJ/mol D Single Bonds Multiple Bonds C N O F Si P S a Br 1 H 436 413 391 463 565 318 322 347 C 413 346 305 358 485...
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
Calculate the enthalpy of the reaction below using the given bond energies. Cl2 + Br2 → 2 BrCI Bond Energy (kJ/mol) CI-CI 242 Br-Br 193 Br-CI 218 0 -267 kj 217 kJ 0-1 kj 653 kJ
Bond Dissociation Energies (for A-B Bond broken AH, kJ/mol Bond broken → A A4, kJ/mol + B) Bond broken mo H-H CH3CH2CH2-H (CH3)2CH-H (CH3)3C-H 436 423 413 400. H-Br 366 CH3CH2CH2-Br 294 (CH3)2CH-Br 298 (CH3)3C-Br292 Br-Br 193 H-CI 432 CH3CH2CH2-CI 354 (CH3)2CH-CI 355 (CH3)3C-CI 349 CI-CI 243 Alkane halogenation is a two-step reaction, as shown below. Using the table of bond dissociation energies, calculate the enthalpy of each step and the enthalpy of the overall reaction. Step 1: Number CH3CHCH3...
Using average bond enthalpies (linked above), estimate the enthalpy change for the following reaction: 2CO(g) + 2NO(g)2CO2(g) + N2(g) kJ Bond Bond Energy (kJ/mol) C=C 602 H-H 436 C-H 413 C-C 346 Using average bond enthalpies (linked above), estimate the enthalpy change for the following reaction: I2(g) + Cl2(g)2ICl(g) kJ Using the values of bond energy from the table above, estimate the enthalpy change for the following reaction: C2H4(g) + H2(g) C2H6(g) kJ