Question

Use the following reaction enthalpies to determine the reaction enthalpy for 2 HCl(g) + F2(g) →...

Use the following reaction enthalpies to determine the reaction enthalpy for 2 HCl(g) + F2(g) → 2 HF(g) + Cl2(g).

4 HCl(g) + O2(g) → 2 H2O(l) + 2 Cl2(g) ΔHrxn = - 202.4 kJ/mol rxn

1/2 H2(g) + 1/2 F2(g) → HF(g) ΔHrxn = - 271.0 kJ/mol rxn

H2(g) + 1/2 O2(g) → H2O(l) ΔHrxn = - 285.8 kJ/mol rxn

Science   Chemistry   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

0 0
Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Log In

Sign Up

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
Use Hess's Law to calculate the enthalpy of reaction, ΔH rxn, for the reaction in bold...
Use Hess's Law to calculate the enthalpy of reaction, ΔH rxn, for the reaction in bold below given the following chemical steps and their respective enthalpy changes. Show ALL work! 2 C(s) + H2(g) → C2H2(g) ΔH°rxn = ? 1. C2H2(g) + 5/2 O2(g) → 2CO2 (g) + H2O (l) ΔH°rxn = -1299.6 kJ 2. C(s) + O2(g) → CO2 (g) ΔH°rxn = -393.5 kJ 3. H2(g) + ½ O2(g) → H2O (l) ΔH°rxn = -285.8 kJ
The enthalpy of the following reactions: COCl2 (g) + H2O (l)= CH2Cl2 (l) + O2 (g)...
The enthalpy of the following reactions: COCl2 (g) + H2O (l)= CH2Cl2 (l) + O2 (g) delta H = 19 kJ ; HCl (g)= 1/2 H2 (g) + 1/2 Cl2 (g) delta H = 92 kJ; CH2Cl2 (l) + H2 (g) + 3/2 O2 (g) = COCl2 (g) + 2 H2O (l) delta H = -161 kJ. Use these reactions to create a reaction pathway for the reaction of chlorine with water as shown below. Then use Hess;s law to...
Calculate the standard enthalpy of reaction for 2 C(graphite) + 3 H2(g) C2H6(g) Given the following...
Calculate the standard enthalpy of reaction for 2 C(graphite) + 3 H2(g) C2H6(g) Given the following standard enthalpy of combustion data, ∆H˚comb (C(graphite) = –393.5 kJ·mol–1 H2(g) + ½ O2(g) H2O(l) ∆H˚rxn = –285.8 kJ·mol–1 2 C2H6(g) + 7 O2(g) 4 CO2(g) + 6 H2O(l) ∆H˚rxn = –3119.6 kJ·mol–1 (a) –84.6 kJ·mol–1 (b) 2440.2 kJ·mol–1 (c) –3799.0 kJ·mol–1 (d) –224.5 kJ·mol–1(e) not enough information provided
9. Use the following experimentally derived combustion data to calculate the standard molar enthalpy of formation...
9. Use the following experimentally derived combustion data to calculate the standard molar enthalpy of formation (ΔH°f ) of liquid methanol (CH3OH) from its elements. 2 CH3OH(l) + 3 O2(g) → 2 CO2(g) + 4 H2O(l)     ΔH°rxn = −1452.8 kJ C(graphite) + O2(g) → CO2(g)                               ΔH°rxn = −393.5 kJ 2 H2(g) + O2(g) → 2 H2O(l)                                     ΔH°rxn = −571.6 kJ (1) −238.7 kJ/mol    (2) 487.7 kJ/mol       (3) −548.3 kJ/mol    (4) 20.1 kJ/mol         (5) 47.1 kJ/mol
6-56) Use standard enthalpies of formation to calculate ΔHrxn° for each reaction. a) 2 H2S(g) +...
6-56) Use standard enthalpies of formation to calculate ΔHrxn° for each reaction. a) 2 H2S(g) + 3 O2(g) ⇒2 H2O(l) + 2 SO2(g) b) SO2(g) + 12 O2(g) ⇒ SO3(g) c) C(s) + H2O(g) ⇒ CO(g) + H2(g) d) N2O4(g) + 4 H2(g) ⇒ N2(g) + 4 H2O(g)
Calculate the enthalpy change (ΔrH) for the reaction below,         N2(g) + 3 F2(g) → 2...
Calculate the enthalpy change (ΔrH) for the reaction below,         N2(g) + 3 F2(g) → 2 NF3(g) given the bond enthalpies of the reactants and products. Bond Bond Enthalpy (kJ/mol×rxn) N–N 163 N=N 418 N≡N 945 F–F 155 N–F 283
Given the following information below, use Hess’s Law to calculate the enthalpy of formation for sodium...
Given the following information below, use Hess’s Law to calculate the enthalpy of formation for sodium oxide: Na (s)     +      HCl (l)  à    NaCl (aq) + ½ H2 (g)                ∆HRx = -393.1 kJ/mol Na2O (s)     +     2 HCl (l)  à 2 NaCl (aq)   + H2O              ∆HRx = -675.2 kJ/mol H2 (g)       +      ½ O2 (g)  à    H2O (g)                              ∆HRx = -288.1 kJ/mol 2 Na (s)       +       ½ O2 (g)   à   Na2O (s)                          ∆HRx =    __________ kJ/mol Calculated Heat of Reaction is....? (Put your answer in...
Using the bond enthalpies in the Average Bond Enthalpies table, determine the approximate enthalpy (in kJ)...
Using the bond enthalpies in the Average Bond Enthalpies table, determine the approximate enthalpy (in kJ) for each of the following reactions. (Assume the average bond enthalpy of the Cl–F bond is 254 kJ/mol.) C) 2 CH3(C=O)H(g) + 5 O2(g) → 4 CO2(g) + 4 H2O(g)
Use the standard reaction enthalpies given below to determine ΔH°rxn for the following reaction: 2 S(s)...
Use the standard reaction enthalpies given below to determine ΔH°rxn for the following reaction: 2 S(s) + 3 O2(g) → 2 SO3(g) ΔH°rxn = ? Given: SO2(g) → S(s) + O2(g) ΔH°rxn = +296.8 kJ 2 SO2(g) + O2(g) → 2 SO3(g) ΔH°rxn = -197.8 kJ Please explain in detail.
1.) Using enthalpies of formation, calculate the standard change in enthalpy for the thermite reaction. The...
1.) Using enthalpies of formation, calculate the standard change in enthalpy for the thermite reaction. The enthalpy of formation of Fe3O4 is −1117 kJ/mol. 8 Al(s) + 3 Fe3O4(s) → 4 Al2O3(s) + 9 Fe(s) 2. a) Nitroglycerin is a powerful explosive, giving four different gases when detonated. 2 C3H5(NO3)3(l) → 3 N2(g) + 1/2 O2 (g) + 6 CO2(g) + 5 H2O(g) Given that the enthalpy of formation of nitroglycerin, ΔHf°, is −364 kJ/mol, calculate the energy (heat at...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT