Question

Consider the reaction, 2 NF3 (g) ' 2 N2 (g) + 3 F2 (g) ΔH° =...

Consider the reaction, 2 NF3 (g) ' 2 N2 (g) + 3 F2 (g)

ΔH° = + 260.8 kJ, ΔS° = + 278.5 J/K

At what temperature will the system be at equilibrium, when all gases are present at 1 atm (standard pressure conditions)?

Calculate the value of the equilibrium constant for the reaction above at 500.0°C.

Homework Answers

Answer #1

1)

At equilibrium, deltaGo = 0

deltaGo = 0.0 KJ

deltaHo = 260.8 KJ

deltaSo = 278.5 J/K

= 0.2785 KJ/K

we have below equation to be used:

deltaGo = deltaHo - T*deltaSo

0.0 = 260.8 - T *0.2785

T = 936 K

Answer: 936 K

2)

T= 500.0 oC

= (500.0+273) K

= 773 K

we have below equation to be used:

deltaGo = deltaHo - T*deltaSo

deltaGo = 260.8 - 773.0 * 0.2785

deltaGo = 45.5195 KJ

deltaG = 45519.5 J

we have below equation to be used:

deltaG = -R*T*ln Kc

45519.5 = - 8.314*773.0* ln(Kc)

ln Kc = -7.0828

Kc = 8.39*10^-4

Answer: 8.39*10^-4

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
For the reaction 2C2H6(g) + 7O2(g) ----> 4CO2(g) + 6H2O(g) ΔH° = -2855.4 kJ and ΔS°...
For the reaction 2C2H6(g) + 7O2(g) ----> 4CO2(g) + 6H2O(g) ΔH° = -2855.4 kJ and ΔS° = 92.7 J/K The maximum amount of work that could be done when 2.39 moles of C2H6(g) react at 349 K, 1 atm is ____ kJ. Assume that ΔH° and ΔS° are independent of temperature.
Consider the following reaction: 2AgCl(s) → 2Ag(s) + Cl2(g); ΔH° = 127.1 kJ; ΔS° = 115.7...
Consider the following reaction: 2AgCl(s) → 2Ag(s) + Cl2(g); ΔH° = 127.1 kJ; ΔS° = 115.7 J/K at 298 K Suppose 59.4 g of silver(I) chloride is placed in a 63.1 L vessel at 298 K. What is the equilibrium partial pressure of chlorine gas? (R = 0.0821 L · atm/(K · mol) = 8.31 J/(K · mol)) A.5.7 × 10-17 atm B.0.95 atm C.5.1 × 10-23 atm D.0.081 atm E.0.16 atm
1)Use standard thermodynamic data (in the Chemistry References) to calculate G at 298.15 K for the...
1)Use standard thermodynamic data (in the Chemistry References) to calculate G at 298.15 K for the following reaction, assuming that all gases have a pressure of 19.31 mm Hg. 2N2(g) + O2(g)2N2O(g) G = ? kJ/mol 2)Using standard thermodynamic data (linked), calculate the equilibrium constant at 298.15 K for the following reaction. C2H4(g) + H2O(g)CH3CH2OH(g) K = ? 3) Calculate the temperature (in kelvins) at which the sign of G° changes from positive to negative for the reaction below. This...
1.      Calculate the standard free energy change at 500 K for the following reaction. Cu(s) +...
1.      Calculate the standard free energy change at 500 K for the following reaction. Cu(s) + H2O(g) à CuO(s) + H2(g) ΔH˚f (kJ/mol) S˚ (J/mol·K) Cu(s)    0    33.3    H2O(g)    -241.8    188.7    CuO(s)    -155.2    43.5    H2(g)     0    130.6 2.      When solid ammonium nitrate dissolves in water, the resulting solution becomes cold. Which is true and why? a.      ΔH˚ is positive and ΔS˚ is positive b.      ΔH˚ is positive and ΔS˚...
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
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...
Please solve step by step for Part D Consider the Haber synthesis of gaseous NH3 (ΔH∘f=−46.1kJ/mol...
Please solve step by step for Part D Consider the Haber synthesis of gaseous NH3 (ΔH∘f=−46.1kJ/mol ;ΔG∘f=−16.5kJ/mol) : N2(g)+3H2(g)→2NH3(g) Part A Use only these data to calculate ΔH∘ and ΔS∘ for the reaction at 25 ∘C. Express your answers using three significant figures separated by a comma. ΔH∘, ΔS∘ = -92.2,-199   kJ, J/K   Part D. What are the equilibrium constants Kp and Kc for the reaction at 370 K ? Assume that ΔH∘ and ΔS∘ are independent of temperature.​ Express...
Consider the reaction given below. H2(g) + F2(g) 2 HF(g) (a) Using thermodynamic data from the...
Consider the reaction given below. H2(g) + F2(g) 2 HF(g) (a) Using thermodynamic data from the course website, calculate G° at 298 K. kJ (b) Calculate G at 298 K if the reaction mixture consists of 6.6 atm of H2, 3.8 atm of F2, and 0.43 atm of HF.
Diatomic and atomic fluorine gas exists in equilibrium according to the following reaction F2(g) -><- 2F(g)...
Diatomic and atomic fluorine gas exists in equilibrium according to the following reaction F2(g) -><- 2F(g) (a) The standard molar Gibbs free energy of reaction, ∆rG at 298 K is 5.25 kJ mol−1 at 298 K. Use this information to calculate the equilibrium constant for the reaction. (b) Calculate the extent of reaction, ξ, for this reaction if 1.0 mole of F2 and 0.0 moles of F are present initially. The equilibrium pressure is 1.3 bar.
he thermodynamic properties for a reaction are related by the equation that defines the standard free...
he thermodynamic properties for a reaction are related by the equation that defines the standard free energy, ΔG∘, in kJ/mol: ΔG∘=ΔH∘−TΔS∘ where ΔH∘ is the standard enthalpy change in kJ/mol and ΔS∘ is the standard entropy change in J/(mol⋅K). A good approximation of the free energy change at other temperatures, ΔGT, can also be obtained by utilizing this equation and assuming enthalpy (ΔH∘) and entropy (ΔS∘) change little with temperature. Part A For the reaction of oxygen and nitrogen to...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT