Question

The standard free energy of formation of nitric oxide, NO, at 800. K (roughly the temperature...

The standard free energy of formation of nitric oxide, NO, at 800. K (roughly the temperature in an automobile engine during ignition) is 72.0 kJ/mol. Δf H (N2) and Δf H (O2) =0.

Calculate the equilibrium constant for the reaction: N2(g) + O2(g) => 2NO(g) at 800. K. (R = 8.31 J/(K · mol)) 2NO(g)

a. 7.0 x 10^–10

b. 7.0 x 10^–9

c. 4 x 10^-10

d. 4 x 10^5

e. 6.8 x 10^–6

Science   Chemistry   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

Standard free energy formation of NO =

=

For 2 moles standard free energy of formation of NO = 144*103 J

Relation between standard free energy and equilibrium constant

, where R= 8.314 J/K.mol and T = 800 K

K = 4*10-10

So answer is (c)

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
The equilibrium constant, Kc, for the formation of nitrosyl chloride from nitric oxide and chlorine. 2NO(g)...
The equilibrium constant, Kc, for the formation of nitrosyl chloride from nitric oxide and chlorine. 2NO(g) + Cl2(g) ⇌ 2NOCl(g) is 6.5 ×10^4 at 35°C. In which direction will the reaction proceed to reach equilibrium if the starting concentrations of NO, Cl2, and NOCl are 6.8 ×10^−3 M, 7.5 ×10^−4 M, and 7.4 M respectively?
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 the reaction at 298 K: N2 (g) + 2 O2 (g) --> 2 NO2 (g)...
Consider the reaction at 298 K: N2 (g) + 2 O2 (g) --> 2 NO2 (g) The value of ΔHo formation of NO2 (g) is known to be 34.0 kJ/mol, while the value of K is 5.86 x 10-19. Determine the absolute entropy of N2 (g) at 298 K if So O2 = 205 J/K mol and So NO2 = 240 J/K mol. (a) 76.3 J/K (b) 133 J/k (c) 190 J/K (d) 304 J/K (e) 507 J/K
Ammonia is burned to form nitric oxide in the following reaction: 4NH3 + 5O2 ----> 4NO...
Ammonia is burned to form nitric oxide in the following reaction: 4NH3 + 5O2 ----> 4NO + 6H2O The Fractional conversion of oxygen is 0.500 and the inlet flow rates of NH3 is 10 mol/h Oxygen is supplied using air (assume 79:21 - N2:O2) fed to reactor at rate of 710 g/h (a) How much oxygen is fed to the reactor (in mol/h)? (b) Which reactan is in excess and by how much (in %)? (c) Calculate the exit molar...
Use the free energies of formation given below to calculate the equilibrium constant (K) for the...
Use the free energies of formation given below to calculate the equilibrium constant (K) for the following reaction at 298 K. 2 HNO3(aq) + NO(g) → 3 NO2(g) + H2O(l) K = ? ΔG°f (kJ/mol) -110.9 87.6 51.3 -237.1 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 ΔG°rxn using the following information. 2 H2S(g) + 3 O2(g) → 2...
The Ostwald process for the commercial production of nitric acid from ammonia and oxygen involves the...
The Ostwald process for the commercial production of nitric acid from ammonia and oxygen involves the following steps: 4NH3(g)+5O2(g)------->4NO(g)+6H2O(g) -908 kj/mol (delta H) 2NO(g)+O2(g)----------->2NO2(g) -112 kj/mol 3NO2(g)+H2O(l)-------->2HNO3(aq)+NO(g) -140 kj/mol Write the overall equation for the production of nitric acid by the Ostwald process by combining the preceding equations (Water is also a product). So i know the answer is this... "Multiply the equations so that the coefficients of the N-products become the same as the N-educts of the following line....
calculate the standard free energy change delta G for reaction N2 (g) +3H2(g)—>2NH3 N2 delta H=0.00kj...
calculate the standard free energy change delta G for reaction N2 (g) +3H2(g)—>2NH3 N2 delta H=0.00kj mol^-1s=+191.5J mol^-1K^-1 H2 delta H=0.00kj mol^-1,s = +130.6j mol^-1 k-1 NH3 delta H=-46.0kj mol^-1,s =192.5 J mol^-1 k-1 A. +112.3 kJ B.-87.6kJ C.-7.4kJ D.-32.9 kJ E.-151.1kJ
Under standard conditions, the free energy of formation (ΔGof) of CO2 ­(g) is -394 kJ/mol. C...
Under standard conditions, the free energy of formation (ΔGof) of CO2 ­(g) is -394 kJ/mol. C (s) + O2 (g) → CO2 (g) Assuming the temperature remains 25 oC and the partial pressure of O2 (g) remains 1 atm, what would be the value of ΔG for this reaction when the partial pressure of CO2 ­(g) is 7.88 x 10-3 atm?
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...
The Ostwald process for the commercial production of nitric acid from ammonia and oxygen involves the...
The Ostwald process for the commercial production of nitric acid from ammonia and oxygen involves the following steps: 4NH3(g)+5O2(g)------->4NO(g)+6H2O(g) -908 kj/mol (delta H) 2NO(g)+O2(g)----------->2NO2(g) -112 kj/mol 3NO2(g)+H2O(l)-------->2HNO3(aq)+NO(g) -140 kj/mol Write the overall equation for the production of nitric acid by the Ostwald process by combining the preceding equations (Water is also a product). So i know the answer is this... "Multiply the equations so that the coefficients of the N-products become the same as the N-educts of the following line....
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT