Question

N2(g) + H2(g) → NH3(g)                                    Ammonia production is

N2(g) + H2(g) → NH3(g)                                   

Ammonia production is one example of an industrial product. It is largely used for fertilizers. Since it has great significance, out of curiosity, please calculate

(a) the standard reaction entropy = _______________ J/K.mol. 4 sig. figures normal format (default normal format).

Given:

Smϴ(NH3,g) = 192.45 J/K.mol

Smϴ(N2,g) = 191.61 J/K.mol

Smϴ(H2,g) = 130.68 J/K.mol

ΔfHϴ(NH3,g) = -46.11 kJ/mol

(b) the change in entropy of the surroundings (at 298 K) of the reaction by initially calculating the enthalpy of formation of ammonia.

ΔSsurr = ________________ J/K.mol.

(c) the standard Gibbs energy of the reaction in kJ/mol.

Science   Chemistry   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

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
Ammonia is formed by the Haber process according to the following reaction: N2(g) + 3H2(g) ⇌...
Ammonia is formed by the Haber process according to the following reaction: N2(g) + 3H2(g) ⇌ 2NH3(g) Use the following data table to answer the questions below: Substance: ΔHf (kJ/mol) So (J/(mol*K) N2(g) 0    187.4 H2(g) 0 127.1 NH3(g) -47.3 197.6 Part 1: Using the table in the introduction, calculate the value of ΔH in units of kJ/mol. After, calculate the value of ΔS in units of J/(mol*K). Finally, cCalculate the value of ΔG in units of kJ/mol for...
In the Haber process, ammonia is synthesized from nitrogen and hydrogen: N2(g) + 3H2(g) → 2NH3(g)...
In the Haber process, ammonia is synthesized from nitrogen and hydrogen: N2(g) + 3H2(g) → 2NH3(g) ΔG° at 298 K for this reaction is -33.3 kJ/mol. The value of ΔG at 298 K for a reaction mixture that consists of 1.7 atm N2, 3.2 atm H2, and 0.85 atm NH3 is a) -139.6 b) 0.43 c) -4.63 × 103 d) -44.1 e) -1.08 × 104
The standard enthalpy change for this reaction is -731 kJ/mol at 298 K. 2 N2(g) +...
The standard enthalpy change for this reaction is -731 kJ/mol at 298 K. 2 N2(g) + 4 H2(g) + 3 O2(g) = 2 NH4NO3(s) ΔrH° = -731 kJ/mol Calculate the standard enthalpy change for the reaction N2(g) + 2 H2(g) + 3/2 O2(g) = NH4NO3(s) at 298 K.
A: 2 NH3 (g) + 46 kJ <-> N2 (g) + 3 H2 (g) For the...
A: 2 NH3 (g) + 46 kJ <-> N2 (g) + 3 H2 (g) For the reaction at equilibrium given above, give 2 ways that you can shift the equibrium to the left. B: 2 NH3(g) + 46 kJ <-> N2(g) + 3 H2(g) For the reaction at equilbrium given above, calculate the numeric value of Kc if the concentrations at equilibrium are 0.50 M NH3(g) , 0.44 M N2(g), and 0.20 M H2(g). C: 2 NH3(g) + 46 kJ...
A sample of 0.60 moles of N2 reacts with 0.35 moles of H2 to form ammonia...
A sample of 0.60 moles of N2 reacts with 0.35 moles of H2 to form ammonia (NH3). If ammonia is the only product, what mass of ammonia is formed? Molar masses: H2=2.016 g/mol, N2=28.02 g/mol, NH3=17.03 g/mol.
The reaction N2 + 3 H2----> 2 NH3 is used to produce ammonia. When 450.0 g...
The reaction N2 + 3 H2----> 2 NH3 is used to produce ammonia. When 450.0 g of hydrogen was reacted with nitrogen, the percent yield you achieved was 30.8%. What was the mass of ammonia produced?
How much ammonia can be synthesized from 5.22 kg of H2 and 31.5 kg of N2...
How much ammonia can be synthesized from 5.22 kg of H2 and 31.5 kg of N2 based on the following reaction: 3 H2(g) + N2(g) à 2 NH3(g) (H2= 2.02 g/mol, N2= 28 g/mol, NH3 = 17.02 g/mol) A.15.5 kg B.29.3 kg C.38.3 kg D.65.9 kg
hydrogen gas, H2, reacts with nitrogen gas,N2, to form ammonia gas , NH3 according to the...
hydrogen gas, H2, reacts with nitrogen gas,N2, to form ammonia gas , NH3 according to the equation... 3H2+N2 --->2NH3 1.how many grams of NH3 can be produced from 3.42 mol of N2 and excess H2 2. how many grams of H2 are needed to produce 14.93 g of NH3 ? 3. How many molecules (not moles) of NH3 are produced from 6.04*10^-4 g of H2 ?
1) For which of the following processes does entropy decrease? A. H2(g) + Cl2(g)   →   2HCl(g)...
1) For which of the following processes does entropy decrease? A. H2(g) + Cl2(g)   →   2HCl(g) B. N2(g) + 3H2(g)   → 2NH3(g) C. Making amorphous glass from crystalline SiO2 (quartz) D. CH3OH(l) → CH3OH(aq) 2) Use the values provided in the table to calculate the standard free energy change for the following reaction at 298 K:   2H2O2(g)  → 2H2O(g) + O2(g)   Substance ∆Gf° (kJ/mol) at 298 K H2O(g) −228 H2O2(g) −105 A −666 kJ B +666 kJ C +246 kJ D −246...
Ammonia equilibrium N2 (g) + 3 H2 (g) <-> 2 NH3 (g) is at equilibrium when...
Ammonia equilibrium N2 (g) + 3 H2 (g) <-> 2 NH3 (g) is at equilibrium when additional nitrogen is added under specific conditions, where T and P held constant, further dissociation of ammonia occurs A) Explain why. B) What conditions are needed? C) Why would adding more H2 produce the same result? This is Physical Chemistry homework. Thank you!
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT