Question

For which of the following reactions does ΔHrxn represent an enthalpy of formation? 2N2(g) + 3O2(g)...

For which of the following reactions does ΔHrxn represent an enthalpy of formation?

2N2(g) + 3O2(g) => 2NO2(g) + 2NO(g)

N2(g) + O2(g) => 2NO(g)

2NO2(g) => N2O4(g)

N2(g) + 2O2(g) => 2NO2(g)

Science   Chemistry   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

enthapy of formation is the enthalpy change when there is formation of one mol of a substance with its constituent elements in their standard state.

Chemical reactions 1,2 and 4  doesn't represent enthalpy of formation because there is formation of 2 mol of product instead of one mol.

In Chemical reaction 2, reactants are not in standard state ie in N2(g) and O2(g) . Therefore, it is also doesn't represent enthalpy of formation.

Therefore, none of reaction' s ΔHrxn represent enthalpy of formation.

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
30) Given the following reactions and their enthalpy changes, calculate the enthalpy change for 2NO2(g) --->...
30) Given the following reactions and their enthalpy changes, calculate the enthalpy change for 2NO2(g) ---> N2O4(g) Equations Change in Heat Energy N2(g) + 2O2(g) ---> 2NO2 (g) +67.8kJ N2(g) + 2O2(g) ---> N2O4(g) +9.67kJ 32) Calculate ΔH for the process Hg2Cl2(s) ---> 2Hg(l) + Cl2(g) from the following information: Hg(l) + Cl2(g) --> HgCl2(s) ΔH = - 224kJ Hg(l) + HgCl2(s) ---> Hg2Cl2(s) ΔH = - 41.2kJ
Calculate the enthalpy of the reaction 2NO(g)+O2(g)→2NO2(g) given the following reactions and enthalpies of formation: 12N2(g)+O2(g)→NO2(g),   ΔH∘A=33.2...
Calculate the enthalpy of the reaction 2NO(g)+O2(g)→2NO2(g) given the following reactions and enthalpies of formation: 12N2(g)+O2(g)→NO2(g),   ΔH∘A=33.2 kJ 12N2(g)+12O2(g)→NO(g),  ΔH∘B=90.2 kJ
Calculate the enthalpy change for the following reaction, in kJ mol-1 N2O4(g) + Cl2(g) →  2NOCl(g) +...
Calculate the enthalpy change for the following reaction, in kJ mol-1 N2O4(g) + Cl2(g) →  2NOCl(g) + O2(g) given the following data:                                       ∆H (kJ mol-1) 2NOCl(g)  → 2NO(g) + Cl2(g)                              +75.56 2NO(g) + O2(g)  → 2NO2(g)                                -113.05 2NO2(g)     → N2O4(g )                                         -58.03
Based on the standard free energies of formation, which of the following reactions represent a feasible...
Based on the standard free energies of formation, which of the following reactions represent a feasible way to synthesize the product? A. N2(g)+H2(g)→N2H4(g); ΔG∘f=159.3 kJ/mol B. N2(g)+3H2(g)→2NH3(g); ΔG∘f=−33.30 kJ/mol C. N2(g)+O2(g)→2NO(g); ΔG∘f=173.2 kJ/mol D. 2SO(g)+O2(g)→2SO2(g); ΔG∘f=−600.4 kJ/mol Drag the appropriate items to their respective bins. feasible synthesis- not a feasible synthesis-
Consider these reactions and their corresponding K's. 1/2N2+ O2 yields NO2 K1 2NO2 yields 2NO +...
Consider these reactions and their corresponding K's. 1/2N2+ O2 yields NO2 K1 2NO2 yields 2NO + O2 K2 NOBr yields NO + 1/2Br2   K3 Express the K value for the reaction below in terms of K1, K2 and K3 1/2N2+ 1/2O2 + 1/2Br2 yields NOBr K=?
Read Examples 5.11 and 5.12, then determine which of the following reactions have the same ΔHrxn...
Read Examples 5.11 and 5.12, then determine which of the following reactions have the same ΔHrxn ° and ΔHf ° . a) 2 CO(g) + O2(g)  2 CO2(g) b) 3/2 H2(g) + 1/2 N2(g)  NH3(g) c) H2S (g) + 2 O2(g)  H2SO4(l) (ans: b) ***Explain why the other two reactions above do not represent heat of formation equations
Find ΔG∘rxn for the reaction: N2O(g)+NO2(g)→3NO(g) Use the following reactions with known ΔG values: 2NO(g)+O2(g)→2NO2(g)ΔG∘rxn=−71.2kJ N2(g)+O2(g)→2NO(g)ΔG∘rxn=+175.2kJ...
Find ΔG∘rxn for the reaction: N2O(g)+NO2(g)→3NO(g) Use the following reactions with known ΔG values: 2NO(g)+O2(g)→2NO2(g)ΔG∘rxn=−71.2kJ N2(g)+O2(g)→2NO(g)ΔG∘rxn=+175.2kJ 2N2O(g)→2N2(g)+O2(g)ΔG∘rxn=−207.4kJ
Would increasing the volume of the container for each of the following reactions at equilibrium cause...
Would increasing the volume of the container for each of the following reactions at equilibrium cause the system to shift in the direction of the products or the reactants? Part A 2NH3(g)???3H2(g)+N2(g) A. Increasing the volume will shift the system in the direction of the products. B. Increasing the volume will shift the system in the direction of the reactants. C. Increasing the volume will not shift the equilibrium. Part B N2(g)+O2(g)???2NO(g) A. Increasing the volume will shift the system...
Use the information in the table below to determine DGofor the reaction 2NH3(g) + 2O2(g) -->...
Use the information in the table below to determine DGofor the reaction 2NH3(g) + 2O2(g) --> N2O(g) + 3H2O(l) DGo (kJ) N2(g) + 3H2(g) --> 2NH3(g) -33.0 4NH3(g) + 5O2(g) --> 4NO(g) + 6H2O(l) -1010.0 N2(g) + O2(g) --> 2NO(g) 174.9 N2(g) + 2O2(g) --> 2NO2(g) 102.6 2N2(g) + O2(g) --> 2N2O(g) 204.2
Use tabulated standard molar enthalpy changes of formation to calculate Delta H rxn for the following...
Use tabulated standard molar enthalpy changes of formation to calculate Delta H rxn for the following (unbalanced) reactions: SHOW WORK a. N2O4 (g) + H2 (g) --> N2 (g) + H2O(g) b. H2S (g) + O2 (g) --> SO2 (g) + H2O(g) c. Fe2O3 (s) + HCl(g) --> FeCl3 (s) + H2O(g)
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT