Given the ΔGf for N2O(g) = 108.8 kJ/mol. Calculate the ΔGdeg in kJ/mol for the reaction:...

Question

Question

Given the ΔGf for N2O(g) = 108.8 kJ/mol. Calculate the ΔGdeg in kJ/mol for the reaction:

2N2O(g)2N2(g) + O2(g).

can someone please explain how to do this?

science chemistry

Answer 1

Answer #1

Answer 2

Similar Homework Help Questions

Calculate the energy produced (kJ) when 54.2 g dinitrogen oxide is decomposed. 2N2O(g) = 2N2(g) +...

Calculate the energy produced (kJ) when 54.2 g dinitrogen oxide is decomposed. 2N2O(g) = 2N2(g) + O2(g) DH = -164.1 kJ N2O 44.01 g/mol Please post steps
Using the Rxs below determine the value of AG° (in kJ) for this reaction. Rx: N2O(g)...

Using the Rxs below determine the value of AG° (in kJ) for this reaction. Rx: N2O(g) + NO2(g) → 3NO(g) + Rx1: 2NO(g) + O2(g) 2NO2(g) AG°= -71.2 kJ Rx2: N2(g) + O2(g) + 2NO(g) AG° = + 175.2 kJ Rx3: 2N2(e) + O2(g) 2N2O(g) AG° = + 207.4 kJ
2N2O(g) → 2N2(g) + O2(g) ∆Hº = –166.7 kJ/mol find the amount of heat that...

2N2O(g) → 2N2(g) + O2(g) ∆Hº = –166.7 kJ/mol find the amount of heat that will be produced when a 2.25 g sample of N2O(g) decomposes into N2 and O2.

Consider the reaction 2 NO2(g) N2O4(g) . (a) Using ΔGf N2O4(g) = 97.79 kJ/mol and ΔGf...

Consider the reaction 2 NO2(g) N2O4(g) . (a) Using ΔGf N2O4(g) = 97.79 kJ/mol and ΔGf NO2(g) = 51.3 kJ/mol, calculate ΔG° at 298 K. ______ kJ (b) Calculate ΔG at 298 K if the partial pressures of NO2 and N2O4 are 0.45 atm and 1.55 atm, respectively. _____ kJ
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) ΔGf° C2H6 (g) = -32.89 kJ/mol; ΔGf° CO2 (g) = -394.4 kJ/mol; ΔGf° H2O (l) = -237.13 kJ/mol
Using the Rxs below determine the value of Delta G o (in kJ) for this reaction...

Using the Rxs below determine the value of Delta G o (in kJ) for this reaction Using the Rxs below determine the value of AGº (in kJ) for this reaction. Rx: N2O(g) + NO2(g) → 3NO(g) Rx1: 2NO(g) + O2(g) → 2NO2(g) AG°= —71.2 kJ Rx2: N2(g) + O2(g) → 2NO(g) AG° = + 175.2 kJ Rx3: 2N2(g) + O2(g) → 2N2O(g) AG° = + 207.4 kJ

The zero order reaction 2N2O→2N2+O2 has the rate constant 5.8×10−4 mol/L/s. If the concentration of N2O...

The zero order reaction 2N2O→2N2+O2 has the rate constant 5.8×10−4 mol/L/s. If the concentration of N2O at t=10 seconds is 0.152 mol/L, what was the initial concentration of N2O?
Given the following reactions N2 (g) + O2 (g) → 2NO (g) ΔH = +180.7 kJ 2N2O...

Given the following reactions N2 (g) + O2 (g) → 2NO (g) ΔH = +180.7 kJ 2N2O (g) → O2 (g) + 2N2 (g) ΔH = -163.2 kJ the enthalpy of reaction for 2N2O (g) → 2NO (g) + N2 (g) is ________ kJ.
Calculate the value of Kp for the reaction $$2N2(g)+O2(g) 2N2O(g) at 298.15 K and 1273 K....

Calculate the value of Kp for the reaction $$2N2(g)+O2(g) 2N2O(g) at 298.15 K and 1273 K. Thermodynamic data for N2O(g) are: ΔH°f = 82.05 kJ/mol; S° = 219.9 J/mol ·K; ΔG°f = 104.2 kJ/mol. Pt 1: 298.1K Pt 2: 1273 K

ΔGf°(I2(g)) = 19 kJ/mol 7. For the reaction H2(g) +12(g) = 2HI(g) K = 50.0 at...

ΔGf°(I2(g)) = 19 kJ/mol 7. For the reaction H2(g) +12(g) = 2HI(g) K = 50.0 at 721 K (a) What is AG at 721 K? (b) What is Kat 25 °C? (AG HI(g) = +1.7 kJ/mol)