Question

Calculate ΔGrxn at 35 ∘C. for the following reactions: 2CH4(g)→C2H6(g)+H2(g) 2NH3(g)→N2H4(g)+H2(g) N2(g)+O2(g)→2NO(g) 2KClO3(s)→2KCl(s)+3O2(g)

Calculate ΔGrxn at 35 ∘C. for the following reactions: 2CH4(g)→C2H6(g)+H2(g) 2NH3(g)→N2H4(g)+H2(g) N2(g)+O2(g)→2NO(g) 2KClO3(s)→2KCl(s)+3O2(g)

Science   Chemistry   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

ΔGrxn = ΔGform products - ΔGform reactants

= -32.1 - (2 * 68.4) KJ/mol

= -168.9 KJ/mol

part b

ΔGrxn= ΔGform products - ΔGform reactants

ΔGrxn= 120.3 - (-2* 16.4) = 153.1 KJ/mol

ΔGform H2= 0 because H2 is standard state of Hydrogen.

part c

ΔGrxn = 2 * ΔGformNO

because nitrogen and oxygen are in their standard states

= 2*86.6 KJ/mol = 137.2 KJ/mol

part d

ΔGrxn = [2ΔGf(KCl (s)) + 3ΔGf(O2 (g))] - [2ΔGf(KClO3 (s))]

[2(-408.32) + 3(0)] - [2(-289.91)] = -236.82 kJ

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
For each of the following reactions, calculate ΔH∘rxn, ΔS∘rxn, ΔG∘rxn at 25 ∘C. State whether or...
For each of the following reactions, calculate ΔH∘rxn, ΔS∘rxn, ΔG∘rxn at 25 ∘C. State whether or not the reaction is spontaneous. If the reaction is not spontaneous, would a change in temperature make it spontaneous? If so, should the temperature be raised or lowered from 25 ∘C? 2NH3(g)→N2H4(g)+H2(g) 2KClO3(s)→2KCl(s)+3O2(g)
Calculate delta G for the following reactions at 25 deg C? (a) N2(g) + O2(g) -----?2NO(g)...
Calculate delta G for the following reactions at 25 deg C? (a) N2(g) + O2(g) -----?2NO(g) (b) H2O(l) ----?H2O(g) (c) 2C2H2(g) + 5O2(g) ---? 4CO2(g) + 2H2O(l)
Given the following data: 2NH3(g) --> N2(g) + 3 H2(g) deltaH* = 92KJ 2H2(g) + O2(g)...
Given the following data: 2NH3(g) --> N2(g) + 3 H2(g) deltaH* = 92KJ 2H2(g) + O2(g) --> 2H20(g) deltaH* = -484KJ Calculate deltaH for the reaction: 2N2(g) + 6H2O(g) --> 3O2(g) + 4NH3(g)
Use standard free energies of formation to calculate ΔG∘ΔG∘ at 25 ∘C∘C for each of the...
Use standard free energies of formation to calculate ΔG∘ΔG∘ at 25 ∘C∘C for each of the following reactions. Substance ΔG∘f(kJ/mol)ΔGf∘(kJ/mol) H2O(g)H2O(g) −−228.6 H2O(l)H2O(l) −−237.1 NH3(g)NH3(g) −−16.4 NO(g)NO(g) 87.6 CO(g)CO(g) −−137.2 CO2(g)CO2(g) −−394.4 CH4(g)CH4(g) −−50.5 C2H2(g)C2H2(g) 209.9 C2H6(g)C2H6(g) −−32.0 Fe3O4(s)Fe3O4(s) −−1015.4 KClO3(s)KClO3(s) −−296.3 KCl(s)KCl(s) −−408.5 Part A C(s,graphite)+2H2(g)→CH4(g)C(s,graphite)+2H2(g)→CH4(g) Express your answer to one decimal place and include the appropriate units. Part B Fe3O4(s)+4H2(g)→3Fe(s)+4H2O(g)Fe3O4(s)+4H2(g)→3Fe(s)+4H2O(g) Express your answer to one decimal place and include the appropriate units. Part C N2(g)+O2(g)→2NO(g)N2(g)+O2(g)→2NO(g) Express your answer...
Calculate ΔGº for the following reactions at 25ºC: (a) N2(g) + O2(g) ---- 2NO(g) (b) H2O(l)...
Calculate ΔGº for the following reactions at 25ºC: (a) N2(g) + O2(g) ---- 2NO(g) (b) H2O(l) ---- H2O(g) (c) 2C2H2(g) + 5O2(g) ----4CO2(g) + 2H2O(l) Plese show clear step by step answers.
For each calculate ∆Hrxn, ∆Srxn, and ∆Grxn, at 25 degrees celsius and state whether or not...
For each calculate ∆Hrxn, ∆Srxn, and ∆Grxn, at 25 degrees celsius and state whether or not the reaction is spontaneous. If it is not, would a change in temperature make it spontaneous? If so, what would the temperature change need to be? a. 2CH4 (g) --> C2H6 (g) + H2 (g) b. 2KClO3(s) --> 2KCl (s) + 3 O2 (g)
chem:1220 ΔS is positive for the reaction ________. A) 2NO (g) + O2 (g) → 2NO2...
chem:1220 ΔS is positive for the reaction ________. A) 2NO (g) + O2 (g) → 2NO2 (g) B) 2N2 (g) + 3H2 (g) → 2NH3 (g) C) C3H8 (g) + 5 O2 (g) → 3CO2 (g) + 4 H2O (g) D) Mg (s) + Cl2 (g) → MgCl2 (s) E) C2H4 (g) + H2 (g) → C2H6 (g)
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)
Given the following chemical equilibria, N2 (g) + O2 (g) <---> 2NO (g) K1=0.641 4NH3 (g)...
Given the following chemical equilibria, N2 (g) + O2 (g) <---> 2NO (g) K1=0.641 4NH3 (g) + 5O2 (g) <---> 4NO (g) + 6H2O (g) K2=29.48 H2 (g) + 1/2O2 (g) <---> H2O (g) K3=74.93 Determine the equilibrium constant for the reaction below: N2 (g) + 3H2 (g) <---> 2NH3 (g) Kc = ???
10​4.  Calculate the net constant value (Knet) for the following reactions: 2NO​N2+O2 ​​ ​Kc=2.4X1030 NO+ ½ Br2NOBr...
10​4.  Calculate the net constant value (Knet) for the following reactions: 2NO​N2+O2 ​​ ​Kc=2.4X1030 NO+ ½ Br2NOBr ​​ Kc=1.4 ½ N2+ ½ O2  + ½ Br2 NOBR ​ Kc net=?
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT