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Bond enthalpy worksheet, Exercises of Chemistry

Chemistry

Bond enthalpy worksheet anglais

Typology: Exercises

2020/2021

Uploaded on 03/04/2021

temascoelchango
temascoelchango 🇺🇸

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Bond Enthalpy Worksheet
Name _________________________
Use bond enthalpy values to calculate the enthalpy change for the following reactions.
1) CH4 (g) + Br2 (g) CH3Br (g) + HBr (g)
2) C2H4 (g) + HBr (g) C2H5Br (g)
3) C4H8 (g) + H2 (g) C4H10 (g)
4) C3H6 (g) + I2 (g) C3H6I2 (g)
5) While burning methane, you collect 3000 KJ of energy. How many grams were burned?
CH4 (g) + 2O2 (g) CO2 (g) + 2H2O (g)
6) If you burn 3 grams of methane to heat a 2L pot of water at 15°C how hot will it get?
(assume no heat is lost to the air)
CH4 (g) + 2O2 (g) CO2 (g) + 2H2O (g)
7) What is the enthalpy change of photosynthesis?
6CO2 + 6H2O C6H12O6 + 6O2
8) How much heat is produced when you burn a 5 gram marshmallow (assume it is all
sucrose (C12H24O11)
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Name _________________________

Use bond enthalpy values to calculate the enthalpy change for the following reactions.

  1. CH 4 (g) + Br 2 (g)  CH 3 Br (^) (g) + HBr (^) (g)
  2. C 2 H 4 (g) + HBr (^) (g)  C 2 H 5 Br (^) (g)
  3. C 4 H 8 (g) + H 2 (g)  C 4 H 10 (g)
  4. C 3 H 6 (g) + I 2 (g) C 3 H 6 I 2 (g)
  5. While burning methane, you collect 3000 KJ of energy. How many grams were burned? CH4 (g) + 2O 2 (g)  CO 2 (g) + 2H 2 O (^) (g)
  6. If you burn 3 grams of methane to heat a 2L pot of water at 15°C how hot will it get? (assume no heat is lost to the air) CH4 (g) + 2O 2 (g)  CO 2 (g) + 2H 2 O (^) (g)
  7. What is the enthalpy change of photosynthesis? 6CO 2 + 6H 2 O  C 6 H 12 O 6 + 6O 2
  8. How much heat is produced when you burn a 5 gram marshmallow (assume it is all sucrose (C 12 H 24 O 11 )

Name _________________________

  1. Hydrogen chloride can react with acetylene in a two-stage addition process to give a saturated product. Calculate the enthalpy change for this reaction using bond enthalpy values from the data. C 2 H 2 (g) +2HCl (^) (g)  C 2 H 4 Cl2 (g)
  2. The data book gives the enthalpy of combustion of ethanol as -1367kJ/mol. Use bond enthalpies to calculate the enthalpy change for this reaction. C 2 H 5 OH (^) (g) + 3O 2 (g)  2CO 2 (g) + 3H 2 O (^) (g)
  3. Calculate the enthalpy of formation for ethane using the enthalpy of sublimation and bond enthalpy values from the data book. 2C (^) (s) +2H 2 (g)  C 2 H 4 (g) 12.The databook quotes the mean bond enthalpy for a carbon-to-carbon double bond (C=C) as 602 kJ/mol. Use the enthalpy of formation given and bond enthalpies from the databook to calculate the enthalpy of the C=C bond in ethene. 2C (^) (s) + 2H 2 (g)  C 2 H 4 (g) Δ H f = 52 kJ/mol

Name _________________________

  1. Use the bond enthalpy values quoted in the data book to calculate the enthalpy change for the hydrogenation of but-1-ene. C4H8 (g) + H2 (g) C4H10 (g)

Name _________________________

  1. Hydrogen chloride can react with acetylene in a two-stage addition process to give a saturated product. Calculate the enthalpy change for this reaction using bond enthalpy values from the data book. C 2 H 2 (g) + 2HCl (^) (g)  C 2 H 4 Cl 2 (g) Bond breaking Bond making 1 mol C≡C = 835 1 mol C–C = 346 2 mol C–H = 2 × 414 = 828 4 mol C–H = 4 × 414 = 1656 2 mol H–Cl = 2 × 428 = 856 2 mol C–Cl = 2 × 326 = 652 Total energy put in = +2519 kJ Total energy given out = –2654 kJ Δ H = 2519 – 2654 = –135 kJ/mol
  2. The data book gives the enthalpy of combustion of ethanol as –1367 kJ mol–1. Use bond enthalpies to calculate the enthalpy change for this reaction. C 2 H 5 OH (^) (g) + 3O 2 (g)  2CO 2 (g) + 3H 2 O (^) (g) Bond breaking Bond making 1 mol C–C = 346 4 mol C=O = 4 × 798 = 3192 5 mol C–H = 5 × 414 = 2070 6 mol H–O = 6 × 458 = 2748 1 mol C–O = 358 1 mol H–O = 458 3 mol O=O = 3 × 497 = 1491 Total energy put in = +4723 kJ Total energy given out = –5940 kJ Δ H = 4723 – 5940 = –1217 kJ/mol
  3. Calculate the enthalpy of formation for ethene using the enthalpy of sublimation and bond enthalpy values from the data book. 2C (^) (s) + 2H 2 (g)  C 2 H 4 (g) Bond breaking Bond making 2 mol C (s) C (g) = 2 × 715 = 1430 1 mol C=C = 602 2 mol H–H = 2 × 432 = 864 4 mol C–H = 4 × 414 = 1656 Total energy put in = +2294 kJ Total energy given out = –2258 kJ Δ H = 2294 – 2258 = + 36 kJ/mol
  4. The data book quotes the mean bond enthalpy for a carbon-to-carbon double bond (C=C) as 602 kJ mol–1. Use the enthalpy of formation given and bond enthalpies from the data book to calculate the enthalpy of the C=C bond in ethene. 2C (^) (s) + 2H2 (g)  C 2 H 4 (g) Δ H f = 52 kJ/mol