Calculate the enthalpy change for the combustion reaction below. 3 CH3OH () O29) → _ C(s) +– CO) _ H2O(g) DHO + xn Single Bond Energies (kJ/mol of bonds) H C S F CI Br Н 436 C 413 346 N 391 305 163 O 463 358 201 146 S 347 272 226 - - F 565 485 283 190 284 155 Cl 432 339 192 218 255 253 242 Br 366 285 201 217 249 216 193 - I 299 213 201 278 208 175 151 ||

Calculate the enthalpy of the reaction below (AHrxn, in kJ) using the bond energies provided. H₂(g) + CH3CH₂C(=O)H → CH3CH₂CH₂OH Single Bond H C N O Multiple Bonds H 432 411 346 386 459 358 C **All values in kJ/mol** 305 167 201 C=C C=C 835 N O 602 C=O C=O C=N C=N 887 615 O=O N=N 142 799 1072 494 942

Use average bond energies to estimate the energy released when 70.0 g CH4 undergoes complete combustion: CH₂(g) +20₂(g) → CO₂(g) + 2H₂O(g) kJ 4

a) Using the balanced equation and the data in the table below, calculate the theoretical enthalpy of combustion. Note: you will need to include the enthalpy of vaporisation for the liquid components which are also given. CH3OH() +1.502(g) → CO2(g) + 2H2O (1) Average Bond Enthalpies (kJ mol‍¹) C-H C-C C-O O=O C=O O-H Enthalpy of Vaporisation (kJ mol-¹) Methanol Water 412 348 358 496 743 463 35 41

Given reaction A + 2B-3C+4D with following standard enthalpies of formation AH:A-10.0 kJ/mol, B-5.0 kJ/mol, C-2.0 kJ/mol, D-12.0 kJ/mol. What is the enthalpy change if 2 moles of B are used in the reaction? O - 68.0 kJ O 68.0 kJ O 34.0 kJ O-34.0 kJ

When 1.42 g of iron reacts with 1.80 g of chlorine, 3.22 g of iron(II) chloride (FeCl2, molar mass = 126.75 g/mol) and 6.8 kJ of heat is produced. What is the enthalpy change for the reaction when 1 mole of iron(II) chloride is produced? round to sig figs

Consider the following reactions: AH = -393.5 kJ (graphite) + 2 AH = -285.8 kJ 2(g) CH,OH + 3/2 0, +2H,0 AH = -726.4 k (1) Choose... Choose... -48.25 Calculate the enthalpy change for the following reaction: 188.7 + 2 H29) CH,OH -37.6 C (graphite) + V½ 0, 10.7 -238.7 39.0 268 11.85 Given the following information: N, bond energy = 941 kJ/mol, F, bond energy = 154 kJ/mol 2 N + 3/2 F AH = -103 kJ/mol 2(g) Choose... Calculate the N-F bond energy (kJ/mol) A ballon originally had a volume of 8.68 L at 258 K and a pressure of 575 mmHg. To what temperature (in K) must the balloon be cooled to reduce its volume to 5.00 L at a pressure of 730 mmHg? Choose... V

Calculate the approximate enthalpy of the following reaction using the data below. 12 "C" atoms joined together in a cyclic (circular) structure with as many Hs connected so that each C atom has 4 bonds in total added to as many 02 atoms (which is O double bonded to another O) as would be required to react gives CO₂ which is a C double bonded to two O atoms and water which is O single bonded to 2 "H" atoms. This reaction needs to be balanced. Data for bond energies in kJ/mol : C single bond C is 347. C single bond H is 414. C double bond O is 736. O double bond O is 498. O single bond H is 464. The Correct answer is -5,736 Can someone explain how can I get to this answer with the steps.

Ozone, O31g2, is a form of elemental oxygen that plays an importantrole in the absorption of ultraviolet radiation in thestratosphere. It decomposes to O21g2 at room temperatureand pressure according to the following reaction:2 O31g2 ¡ 3 O21g2 ΔH = -284.6 kJ(a) What is the enthalpy change for this reaction per moleof O31g2?(b) Which has the higher enthalpy under these conditions,2 O31g2 or 3 O21g2?

Predict the enthalpy change for the reaction below using the thermochemical equations provided. 2 C2H2 + 5 O2 --> 4 CO2 + 2 H2O 4 C + 2 H2 --> 2 C2H2        Δ Hrxn = + 226.7 kJ/mol C + O2 --> CO2                   Δ Hrxn = - 393.5 kJ/mol 2 H2 +  O2 --> 2 H2O         Δ Hrxn = - 571.6 kJ/mol Group of answer choices -2372 kJ/mol -1192 kJ/mol -1919 kJ/mol -738.4 kJ/mol