Question

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

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
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.
Consider the following reaction at 298 K: 2C (graphite) + O2 (g) >>> 2CO (g) Delta...
Consider the following reaction at 298 K: 2C (graphite) + O2 (g) >>> 2CO (g) Delta H = -221.0 kJ Calculate: Delta S(sys) J/K Delta S (surr) J/K Delta S (Univ) J/K
Consider the reaction: 1/2 N2(g) + O2(g)<<<----->>>NO2(g) Write the equilibrium constant for this reaction in terms...
Consider the reaction: 1/2 N2(g) + O2(g)<<<----->>>NO2(g) Write the equilibrium constant for this reaction in terms of the equilibrium constants, Ka and Kb, for reactions a and bbelow: a.) N2O4(g) <-------> 2NO2(g) Ka b.) N2(g) + 2 O2(g) <------> N2O4(g) Kb K =
1. Given the values of So given below in J/mol K and the values of ΔHfo...
1. Given the values of So given below in J/mol K and the values of ΔHfo given in kJ/mol, calculate the value of ΔGo in kJ for the combustion of 1 mole of butane to form carbon dioxide and gaseous water at 298 K. S (C4H10(g)) = 273 S (O2(g)) = 208 S (CO2(g)) = 214 S (H2O(g)) = 189 ΔHfo (C4H10(g)) = -123 ΔHfo (CO2(g)) = -394 ΔHfo (H2O(g)) = -223 2. A particular reaction has a ΔHo value...
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...
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...
Consider the following data at 298 K: Compound ∆Hf° (kJ mol−1) H2S (g) -20.5 H2O (g)...
Consider the following data at 298 K: Compound ∆Hf° (kJ mol−1) H2S (g) -20.5 H2O (g) -242 For the reaction   4 Ag(s) + 2 H2S(g) + O2(g) --> 2 Ag2S(s) + 2 H2O(g)    at a temperature of 25 °C, ∆H° = −507 kJ Calculate the ∆Hf° of Ag2S (s) is (in kJ mol−1): -285.5 -32 -64 + 475
Consider the following reaction at 195 K: 2Cu2O (s) ----> 4 Cu (s) + O2 (g)...
Consider the following reaction at 195 K: 2Cu2O (s) ----> 4 Cu (s) + O2 (g) In one of your laboratory experiments, you determine the equilibrium constant for this process, at 195 K, is 5.060E-84. You are given a table of data that indicates the standard heat of formation (deltaHform) of Cu2O is -170 kJ/mol. Based on this information, what is the stnadard entropy change (deltaSrxn) for this reaction at 195 K? (answer in J/K). Show all work please!
Solve: 2 NO2 (g) + O3 (g) → N2O5 (g) + O2 (g)      ∆Hº = -198...
Solve: 2 NO2 (g) + O3 (g) → N2O5 (g) + O2 (g)      ∆Hº = -198 kJ mol-1RXN     ∆Sº = -168 J K-1        Ozone reacts with nitrogen dioxide according to the equation above. State and explain how the spontaneity of this reaction will vary with increasing temperature. Substance ∆Hºf (kJ mol -1) O3 (g) 143 N2O5 (g) 11
Given the values of K shown below, determine the value of K for the reaction, N2(g)...
Given the values of K shown below, determine the value of K for the reaction, N2(g) + 2 O2(g) <=> 2 NO2(g). N2(g) + O2(g) <=> 2 NO(g) K = 92 NO2(g) <=> NO + 1/2 O2(g) K = 36 the answer is 0.0710 please show work to how to get that answer
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT