Question

Estimate ΔHrxn for the following chemical reaction using the bond enthalpies in the table found here....

Estimate ΔHrxn for the following chemical reaction using the bond enthalpies in the table found here. Report your answer to zero decimal places in standard notation (i.e. 123. kJ *For numbers ending in zero, be sure to include the decimal!*).



C2H2(g) + Cl2(g) → C2H2Cl2(g)

Homework Answers

Answer #1

H rxn = H products - H reactants

H0 for ethene = +52.4 KJ/mole

H0 for Cl2 = 0 KJ/mole

H0 for ethylene chloride = -125.4 KJ/mole

Therefore, H rxn = H products - H reactants

H rxn = -125.4 - (52.4+0) = 73..0 KJ/mole

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
Estimate ΔHrxn for the following chemical reaction using the bond enthalpies in the table found here....
Estimate ΔHrxn for the following chemical reaction using the bond enthalpies in the table found here. Report your answer to zero decimal places in standard notation (i.e. 123. kJ *For numbers ending in zero, be sure to include the decimal!*). C2H2(g) + Cl2(g) → C2H2Cl2(g) ****** I WANT ANONYMOUS C WITH 1,300 ANSWERS TO ANSWER THIS QUSTION !!!!!!!!!
Estimate ΔHrxn for the following chemical reaction using the bond enthalpies in the table found here....
Estimate ΔHrxn for the following chemical reaction using the bond enthalpies in the table found here. Report your answer to zero decimal places in standard notation (i.e. 123. kJ *For numbers ending in zero, be sure to include the decimal!*
4a) Estimate ΔHrxn for the following chemical reaction using the bond enthalpies in the table found...
4a) Estimate ΔHrxn for the following chemical reaction using the bond enthalpies in the table found here. Report your answer to zero decimal places in standard notation (i.e. 123. kJ *For numbers ending in zero, be sure to include the decimal!*). N2H4(g) + O2(g) → N2(g) + 2H2O(g) b) Without doing any calculations, predict the sign of ΔSsys for each of the following processes: (positive or negative) The decomposition of Na2CO3 into its constituent elements (positive or negative) CH4(g) +...
Use the thermodynamic data provided below to estimate the boiling point (in K) of ICl. Report...
Use the thermodynamic data provided below to estimate the boiling point (in K) of ICl. Report your answer to zero decimal places in standard notation (i.e. 123. kJ *For numbers ending in zero, be sure to include the decimal!*). Substance ΔH°f (kJ/mol) S° (J mol-1K-1) ICl (l) -23.89 135.1 ICl (g) 17.78 247.6
1.Using the enthalpies of formation given below, calculate ΔH°rxn in kJ, for the following reaction. Report...
1.Using the enthalpies of formation given below, calculate ΔH°rxn in kJ, for the following reaction. Report your answer to two decimal places in standard notation. H2S(g) + 2O2(g) → SO3(g) + H2O(l) H2S (g): -20.60 kJ/mol O2 (g): 0.00 kJ/mol SO3 (g): -395.77 kJ/mol H2O (l): -285.83 kJ/mol 2. Calculate the amount of heat absorbed/released (in kJ) when 22.54 grams of SO3 are produced via the above reaction. Report your answer to two decimal places, and use appropriate signs to...
Answer the following questions using the chemical reaction and thermochemical information given below: Cl2(g) + C5H8(g)...
Answer the following questions using the chemical reaction and thermochemical information given below: Cl2(g) + C5H8(g) ⇌ 1C5H6(g) + 2HCl(g) ΔHf° (kJ/mol) S° (J mol-1 K-1) C5H6 139.00 274.47 HCl   -92.31 186.90 Cl2 0.00 223.08 C5H8 36.00 289.66 1. Determine ΔG°rx (in kJ) for this reaction at 1474.8 K. Assume ΔH°f and S° do not vary as a function of temperature. Report your answer to two decimal places 2. Determine the equilibrium constant for this reaction. Report your answer to...
The enthalpy change for the following reaction is -185 kJ. Using bond energies, estimate the Cl-Cl...
The enthalpy change for the following reaction is -185 kJ. Using bond energies, estimate the Cl-Cl bond energy in Cl2(g). H2(g) + Cl2(g)------>2HCl(g) ________kJ/mol
Using average bond enthalpies, estimate the enthalpy change for the following reaction: CH4(g) + H2O(g)3H2(g) +...
Using average bond enthalpies, estimate the enthalpy change for the following reaction: CH4(g) + H2O(g)3H2(g) + CO(g) ____kJ
Using average bond enthalpies, estimate the enthalpy change for the following reaction: CH4(g) + 2F2(g)CH2F2(g) +...
Using average bond enthalpies, estimate the enthalpy change for the following reaction: CH4(g) + 2F2(g)CH2F2(g) + 2HF(g) ____kJ
Ammonia is produced directly from nitrogen and hydrogen by using the Haber process. The chemical reaction...
Ammonia is produced directly from nitrogen and hydrogen by using the Haber process. The chemical reaction is N2(g)+3H2(g) ---> 2NH3 (g) (a) Use bond enthalpies to estimate the enthalpy change for the reaction, and tell whether this reaction is exothermic or endothermic (b) Compare the enthalpy change you calculate in (a) to the true enthalpy change as obtained using ∆Hf° values. (∆Hf° of ammonia is -46.19 kJ/mol)
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT