Question

Calculate ΔG (in kJ) at 65 oC for the reaction: N2O(0.0027 atm) + H2(0.43 atm) ↔...

Calculate ΔG (in kJ) at 65 oC for the reaction: N2O(0.0027 atm) + H2(0.43 atm) ↔ N2(890.2 atm) +H2O(l)

Science   Chemistry   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

Reaction quotiet Qp = pN2 / ( pN2O x pH2)           liquids liek H2O not included in eq

Qp = ( 890.2 atm) / ( 0.0027 atm x 0.43 atm)

     = 766753

dGo of reaction = dGo products - dGo reactants

    = dGo N2 + dGo H2O (l) - dGo N2O - dGo H2

    =     0 - 237.14 KJ/mol - 103.8 KJ/mol - 0

           = -340.94 KJ/mol = -340940 J/mol

dG = dGo + RT ln Qp   is formula   where T = 65C = 65+273 = 338 K

dG = -340940 J/mol + ( 8.314 J/molK x 338 K) ln ( 766753)

= -302862 J/mol = -302.86 KJ/mol

= -303 KJ/mol

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
Calculate ?G (in kJ) at 65 oC for the reaction: N2O(0.0086 atm) + H2(0.55 atm) ?...
Calculate ?G (in kJ) at 65 oC for the reaction: N2O(0.0086 atm) + H2(0.55 atm) ? N2(736.6 atm) +H2O(l) Calculate the vapor pressure of Hg at 75 oC (in atm). Hg(l) ? Hg(g) . . . ?Ho = 61.32 kJ and ?So = 98.83 J/K
a) Calculate the equilibrium constant at 17 K for a reaction with ΔHrxno = 10 kJ...
a) Calculate the equilibrium constant at 17 K for a reaction with ΔHrxno = 10 kJ and ΔSrxno = -100 J/K. (Don't round until the end. Using the exponent enlarges any round-off error.) b) Calculate the equilibrium constant at 146 K for the thermodynamic data in the previous question (Notice that Keq is larger at the larger temperature for an endothermic reaction) c) Calculate the equilibrium constant at 43 K for a reaction with ΔHrxno = 10 kJ and ΔSrxno...
Calculate ΔG∘ (in kJ/mol) for the following reaction at 1 atm and 25 °C: C2H6 (g)...
Calculate ΔG∘ (in kJ/mol) for the following reaction at 1 atm and 25 °C: C2H6 (g) + O2 (g)  → CO2 (g) + H2O (l) (unbalanced) ΔHf C2H6 (g) = -84.7 kJ/mol; S C2H6 (g) = 229.5 J/K⋅mol; ΔHf ∘ CO2 (g) = -393.5 kJ/mol; S CO2 (g) = 213.6 J/K⋅mol; ΔHf H2O (l) = -285.8 kJ/mol; SH2O (l) = 69.9 J/K⋅mol; SO2 (g) = 205.0 J/K⋅mol
Calculate the ΔG∘rxn for the reaction using the following information. 4HNO3(g)+5N2H4(l)→7N2(g)+12H2O(l) ΔG∘f(HNO3(g)) = -73.5 kJ/mol; ΔG∘f(N2H4(l))...
Calculate the ΔG∘rxn for the reaction using the following information. 4HNO3(g)+5N2H4(l)→7N2(g)+12H2O(l) ΔG∘f(HNO3(g)) = -73.5 kJ/mol; ΔG∘f(N2H4(l)) = 149.3 kJ/mol; ΔG∘f(N2(g)) = 0 kJ/mol; ΔG∘f(H2O(l)) = -273.1 kJ/mol. Calculate the  for the reaction using the following information. = -73.5 ; = 149.3 ; = 0 ; = -273.1 . -312.9 kJ +110.7 kJ -954.7 kJ -3.298 x 103 kJ +2.845 x 103 kJ
Given the following equation, H2O(g) + CO(g) → H2(g) + CO2(g) ΔG°rxn = -28.6 kJ Calculate...
Given the following equation, H2O(g) + CO(g) → H2(g) + CO2(g) ΔG°rxn = -28.6 kJ Calculate ΔG°rxn for the following reaction. 8 H2O(g) + 8 CO(g) → 8 H2(g) + 8 CO2(g)
1. For the reaction A(g) + 2B(g) ↔ 2C(g) ΔGo = −30.6 kJ. What is the...
1. For the reaction A(g) + 2B(g) ↔ 2C(g) ΔGo = −30.6 kJ. What is the value of ΔG in kJ at 25oC when the pressure of A is 1.3 atm, pressure of B is 1.5 atm, and the pressure of C is 3.7?
1- Above what temperature is the following reaction spontaneous? N2O4(g) ↔ 2 NO2(g) ΔH° = 57.24...
1- Above what temperature is the following reaction spontaneous? N2O4(g) ↔ 2 NO2(g) ΔH° = 57.24 kJ/mol ΔS° = 175.5 J/mol∙K Group of answer choices 326 K 53.2 K 307 K 273 K 2- Predict the sign on ΔG for the following reaction when PI2 = PH2 = 0.01 atm and PHI = 1.0 atm. H2(g) + I2(g) ↔ 2 HI(g) ΔG° = -15.94 kJ/mol & Kp,298K = 620 Group of answer choices ΔG = 0 ΔG > 0 ΔG...
For the reaction: 2 H2 + 2 NO → N2 + 2 H2O the observed rate...
For the reaction: 2 H2 + 2 NO → N2 + 2 H2O the observed rate expression, under some conditions, is: rate = k[H2][NO] Which of the following mechanisms are consistent with these data? Select all that are True. step 1   2 NO → N2O2     (slow)      step 2   N2O2 + H2 → N2O + H2O     (fast)      step 3   N2O + H2 → N2 + H2O     (fast) step 1   NO + NO ⇌ N2O2     (fast)      step 2   N2O2 + H2 → N2 + H2O + O     (slow)      step 3   O + H2...
For the reaction H(g) + H2(g) ↔ (H-H-H)#→ H2(g) + H(g), activation energy Ea= 23 kJ/mol...
For the reaction H(g) + H2(g) ↔ (H-H-H)#→ H2(g) + H(g), activation energy Ea= 23 kJ/mol and the preexponential factor A = 1.5 x 1010 L mol-1s-1 at 298 K. Determine ∆H#, ∆S#, ∆G# and Kc#
The rate law for the reaction: 2H2+2NO--->N2+2H2O is rate=k[H2][NO]^2. Which of the follwing mechanisms can be...
The rate law for the reaction: 2H2+2NO--->N2+2H2O is rate=k[H2][NO]^2. Which of the follwing mechanisms can be ruled out on the basis of the observed rate expression? PLEASE EXPLAIN Mechanism 1: H2+NO--->H2O+N (slow) / N+NO----->N2+O (fast) / O+H2----> N2+O (fast) Mechanism 2: H2+2NO---->N2O+H2O (slow) / N2O+H2---->N2+H2O (fast) Mechanism 3: 2NO<----->N2O2 (fast equilibrium) / N2O2+H2------>N2O+H2O (slow) / N2O+H2------>N2+H2O (fast) PLEASE EXPLAIN WHY.
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT