ZuoTi.Pro
Question

Now write down the manipulated reactions nu uiel CUIT 2) Consider the reaction of methane with hydrogen to give methane CzHs
science   chemistry   
0 0
Add a comment Improve this question Transcribed image text
Next > < Previous
Sort answers by oldest

Homework Answers

Answer #1

Lets number the reaction as 0, 1, 2 from top to bottom
required reaction should be written in terms of other reaction
This is Hess Law
required reaction can be written as:
reaction 0 = +2 * (reaction 1) -1 * (reaction 2)

So, ΔHo rxn for required reaction will be:
ΔHo rxn = +2 * ΔHo rxn(reaction 1) -1 * ΔHo rxn(reaction 2)
= +2 * (-74.9) -1 * (-84.5)
= -65.3 KJ
Answer: -65.3 KJ

0 0
Add a comment
Know the answer?
Add Answer to:
Now write down the manipulated reactions nu uiel CUIT 2) Consider the reaction of methane with...
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. Our experts will answer your question WITHIN MINUTES for Free.
Similar Homework Help Questions

  • Now write down the manipulated reactions mu unsbt nol htemoldo ncb bneo r bn 0oY ob...

    Now write down the manipulated reactions mu unsbt nol htemoldo ncb bneo r bn 0oY ob u 2) Consider the reaction of methane with hydrogen to give methane to abte emc CHe (g)+ H2 (g)2CHa (g) Calculate the value for AH for this reaction given the following thermochemical equations C (s)+2H2 (g) CHa (g) AH =-74.9 kJ 2C (s)+3H2 (g)C2Hs (g) AH = -84.5 kJ bages S ulate the AH° for the following.co ction

  • The direct reaction of methane (CH) with oxygen to give carbon monoxide is hard to accomplish without also producin...

    The direct reaction of methane (CH) with oxygen to give carbon monoxide is hard to accomplish without also producing carbon dioxide. However, we can use a Hess's law calculation to calculate AH,anyway. Calculate AH in kJ for the following reaction from the thermochemical equations given. 35. 2CO(g) + 4H2O() 2CH&(g) +302(g) Use the following thermochemical equations: AH-221.08 kJ 2CO(g) (1) 2C(s)+O2(g) AH=-890.4 kJ CH&g)+202(g) CO2(g)+ 2H20() (2) AH -393.51 kJ CO2(g) C(s)+O2(g) (3)

  • 717)Use the reactions below to calculate the standard change in enthalpy for the reaction of methane...

    717)Use the reactions below to calculate the standard change in enthalpy for the reaction of methane (CH4) with chlorine to form chloroform (CHC13) and hydrochloric acid: CH4(g) + 3Cl2(g) → CHCI3(g) + 3HCI(g) Reaction 1: HCI(g) → H2(g) + 2Cl2(g) AH° = +92.3 kJ Reaction 2: CH4(g) → C(s) + 2H2(g) AH° = +74.8 kJ Reaction 3: C(s) + 3H2(g) + 3/2Cl2(g) →CHCl3(g) AH° = -103.1 kJ x a. +270.2 kl b. +248.6 kJ PC. +64.0 kJ -120.6 kJ -305.2...

  • What is the enthalpy of the following reaction: CH4(g) + NH3(g) à HCN(g) + 3H2(g) Use...

    What is the enthalpy of the following reaction: CH4(g) + NH3(g) à HCN(g) + 3H2(g) Use the data from the following three reactions:             N2(g) + 3H2(g) à 2NH3(g)                               DrH° = -91.8 kJ             C(s) + 2H2(g) à CH4(g)                                    DrH° = -74.9 kJ             H2(g) + 2C(s) + N2(g) à 2HCN(g)                     DrH° = +270.3 kJ 437 kJ 150 kJ 391 kJ 287 kJ 256 kJ

  • DaC. NUL20 1) Find AH, for the reaction 2H2(g) + 2C(s) + O2(g) → C2H5OH(I), using...

    DaC. NUL20 1) Find AH, for the reaction 2H2(g) + 2C(s) + O2(g) → C2H5OH(I), using the following thermochemical data. For Hess's Law, rewrite equations to find out AH. C2H5OH (1) +2 02 (g) → 2 CO2 (g) + 3H20 (1) AH = -875.J C(s) + O2(g) → CO2 (g) AH = -394,51 kJ H2(g) + 12 02 (g) → H20 (1) AH = -285.8 kJ

  • 3. Use the thermochemical equations shown below to determine the enthalpy for the reaction for CH3COOH()2C(s)...

    3. Use the thermochemical equations shown below to determine the enthalpy for the reaction for CH3COOH()2C(s) +2H2(g) + O2(g) 2CO2(g)+ 2H2OI)CH3COOH(l) + 202(B) AH 3484 kJ C(s)+ O2(g)CO2(g) AH= -1576 kJ AH= -2288 kJ 2H2O(I) 2H2(g)+ O2(g)

  • Question 36 of 50 Submit Using the equations N2(g) + 3 H2(g) - 2 NH; (g)...

    Question 36 of 50 Submit Using the equations N2(g) + 3 H2(g) - 2 NH; (g) AH = -91.8 kJ/mol C(s) + 2 H (g) – CH2 (g) AH° = -74.9 kJ/mol H2 (g) + 2c(s) + N2 (g) - 2 HCN (g) AH = 270.3 kJ/mol Determine the enthalpy for the reaction CH, (g) + NH4 () – HCN (g) + 3 H2(g). kJ/mol 1 2 3 C +/- : 0 x 100

  • 3. Calculate the enthalpy of formation of carbon dioxide in the following reaction: C(s) + O2...

    3. Calculate the enthalpy of formation of carbon dioxide in the following reaction: C(s) + O2 (g) – CO2 (g) 213 Use the following equations: a) H20 (0) -- H2(g) + 103() AH',- +285.8 kJ/mol b) CH. (g) -2C (s) + 3H2(g) AH:- +84.7 kJ/mol c) 2CO2(g) +3H() - CH.(g) + (7/2) O, (g) AH,- +1560.7 kJ/mol

  • Review Problem 6.086 Given the following thermochemical equations, 2Cu + S(s) - Cu2S(s) AH° = -79.5...

    Review Problem 6.086 Given the following thermochemical equations, 2Cu + S(s) - Cu2S(s) AH° = -79.5 kJ S(s) + O2(g) → SO2(9) AH = -297 kJ Cu2S(s) + 202(g) → 2CụO(s) + SO2(g) AH° = -527.5 kJ calculate the standard enthalpy of formation (in kilojoules per mole) of Cuo(s). AH°(Cuo(s)) - kJ/mol The number of significant digits is set to 3; the tolerance is +/-2% Show Work is REQUIRED for this question: Open Show Work Review Problem 6.087 Given the...

  • The overall reaction to produce chloroform from methane is CH4(g) + 3Cl2(g) ---> CHCl3(l) + 3HCl(g)....

    The overall reaction to produce chloroform from methane is CH4(g) + 3Cl2(g) ---> CHCl3(l) + 3HCl(g). Use the following intermediate reactions to calculate the enthalpy of the reaction, Hrxn. 1/2 H2(g) + 1/2 Cl2(g) ---> HCl(g)               Hrxn = -92.3 kj C(s) + 2H2(g) ----> CH4(g)                      Hrxn = -74.8 kj C(s) + 1/2 H2(g) + 3/2 Cl2(g) ----> CHCl3(l)    Hrxn = -134.5 kj

ADVERTISEMENT
Free Homework Help App
Download From Google Play
Scan Your Homework
to Get Instant Free Answers
Need Online Homework Help?
Ask a Question
Get Answers For Free
Most questions answered within 3 hours.
ADVERTISEMENT
ADVERTISEMENT
ADVERTISEMENT