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Consider the reaction 2NO2(g)→N2O4(g). ΔG∘ =-5.40 kJ Calculate ΔG at 298 K if the partial pressures of NO2?

source : yahoo.com

Consider the reaction 2NO2(g)→N2O4(g). ΔG∘ =-5.40 kJ Calculate ΔG at 298 K if the partial pressures of NO2?

IMO this is a bit garbled (I’m not blaming you for that!).

I think is is how it’s supposed to be solved.

2NO2(g) → N2O4(g)

Kp = P(products)/P(reactants) = (P(N2O4))/((P(NO2))^2)

Kp = (1.64 atm)/((0.38 atm)^2) = 11.36 atm^-1

Next we need to convert Kp to Kc:

Kp = Kc(RT)^Δngas

So

Kc = Kp/((RT)^Δngas)

Δngas = Mole of gas (product) – Mole of Gas (Reactant) = 1 – 2 = -1

R = 0.08206 L atm K^-1 mol^-1

T = 298 K

Kc = Kp/((RT)^Δngas) = (11.36 atm^-1)/(((0.08206 L atm K^-1 mol^-1)*(298 K))^-1)

Kc = 277.8 L mol-1

Now we use this to calculate ∆G.

∆G = -RT(lnKeq)

http://www.chem.purdue.edu/gchelp/howtosolveit/The…

R = 0.008314 kJ mol^-1 K^-1

T = 298 K

Keq = Kc = 277.8

∆G = -RT(lnKeq)

∆G = -(0.008314 kJ mol^-1 K^-1)*(298 K)*(ln(277.8))

∆G = 13.94 kJ mol^-1

Answered: 2NO2 (g) ⇌ N2O4(g) II. N2(g) +3H2(g) ⇌… | bartleby

Answered: 2NO2 (g) ⇌ N2O4(g) II. N2(g) +3H2(g) ⇌… | bartleby – Chemistry Q&A Library 2NO2 (g) ⇌ N2O4(g) II. N2(g) +3H2(g) ⇌ 2NH3(g) III. PCl5(g) ⇌ PCl3(g) +Cl2(g) Will these equilibria shift towards reactants or products or no change when the volume of the reaction vessel is increased?Calculate the enthalpy of the reaction: 2NO(g) + O2(g) –> 2NO2(g) given the following reactions and enthalpies of formation: 1/2 N2(g) + O2(g) –> NO2(g), delta H *A = 33.2 kJ. 1/2 N2(g) + 1/2O2(g) –> NO(g), delta H *B= 90.2 kJ. Calculate the enthalpy of the reaction: 4B(s)+3O2(g) –> 2B2O3(s) given the following pertinent information:Use Data From Appendix IIB To Calculate The Equilibrium Constants At 25 ∘C For Each Of The Following Reactions.. 2NO2(g)⇌N2O4(g) Express Your Answer Using Two Significant Figures. NO2 (g) H= 33.2 G=51.3 S=240.1 N2O4 (g) H=11.1 G=99.8 S=304.4 Part B 32H2(g)+14P4(g)⇌PH3(g) Express Your Answer Using Two Significant Figures.

Calculate the enthalpy of the reaction: 2NO(g) + O2(g – Consider the reaction 2NO2(g)→N2O4(g). ΔG∘ =-5.40 kJ Calculate ΔG at 298 K if the partial pressures of NO2? Calculate ΔG at 298 K if the partial pressures of NO2 and N2O4 are 0.38atm and 1.64atm , respectively. I solved for the pressure as 1.64-.38^2. then R= 8.314, T is 298 .Calorimetric studies show that the reaction is exothermic. 2NO2(g) N2O4(g) + 14.1 kcal. Based on this information, which one–if any–of the following additional changes would increase the molar concentration at equilibrium of N2O4(g)? decrease the pressure increase the temperature decrease the concentration of NO2(g) stir the reaction mixture2NO2 (g) Equilibrium N2O4 (g)NO2 and N2O4 undergo the reaction shown. When a sealed container of NO2 reaches chemical equilibrium, which must be true?f The maximum number of molecules has been reached.g No N2O4 is present.h The rates of the forward and reverse reactions are equal.j No chemical

Calculate the enthalpy of the reaction: 2NO(g) + O2(g

Solved: 1. Use Data From Appendix IIB To Calculate The Equ – Solution for At a particular temperature, Kp = 0.310 for the reaction N2O4(g) 2NO2(g) A flask containing only N2O4(g) at an initial pressure of 3.70 atm…4(g) to an empty flask and then watch it with time – the gas will slowly go more and more brown as N 2O 4(g) converts to brown NO 2(g).Answer to: Consider the following reversible reaction: N2O4(g) arrow 2NO2(g) a. If we add in more NO2, we will force the reaction further to the….

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