3. (12 pts) Consider the reaction N2(g)+3X2(g) 2NX,(g) H(kJ/mol 0.00.0 210 43 172 S° (J/mol.K) 192...

Question

Question

3. (12 pts) Consider the reaction N2(g)+3X2(g) 2NX,(g) H(kJ/mol 0.00.0 210 43 172 S° (J/mol.K) 192 What is Keq for this reaction at 591 K?

science chemistry

Answer 1

Answer #1

ウブn AS CNX2 (3) 19 2 -478 ー AndAS and ASxn nnolk : 1964981 Tm N-o, △GYxn = _ RTInka @t u.Ala.kv3 un ) -) In kag ___ 19 6498

Answer 2

Similar Homework Help Questions

Find ΔrG for the following (in kJ mol-1) N2 (g) + 3 H2 (g) ⇌ 2...

Find ΔrG for the following (in kJ mol-1) N2 (g) + 3 H2 (g) ⇌ 2 NH3 (g) The conditions for this reaction are: Temp: 298k P - NH3 = 0.95 bar P - H2 = 1.95 bar P - N2 = 1.25 bar NH3(g) ?H ∙(kJ mol-1) = -45.9 ?G ∙(kJ mol-1) = -16.4 S ∙(J K-1 mol-1)192.8 N2(g) ?H ∙(kJ mol-1) = 0 ?G ∙(kJ mol-1) = 0 S ∙(J K-1 mol-1)191.6 H2(g) ?H ∙(kJ mol-1) = 0...
For the reaction N2(g) + O2(g)2NO(g) H° = 180.6 kJ and S° = 24.9 J/K The...

For the reaction N2(g) + O2(g)2NO(g) H° = 180.6 kJ and S° = 24.9 J/K The equilibrium constant for this reaction at 259.0 K is . Assume that H° and S° are independent of temperature.
Consider the following reaction, for which ∆H° = -113.1 kJ/mol and ∆S° = -145.34 J/mol·K. 2NO(g)...

Consider the following reaction, for which ∆H° = -113.1 kJ/mol and ∆S° = -145.34 J/mol·K. 2NO(g) + O2(g) ⇌ 2NO2(g) Assume ∆H° and ∆S° do not vary appreciably with change in temperature. This reaction will only be spontaneous at a temperature _____(i)_____ than ______(ii)_____. (i) lower (ii) 298.15 K (i) higher (ii) 1285 K (i) higher (ii) 1285 K (i) lower (ii) 778 K (i) higher (ii) 778 K

For the reaction N2(g) + O2(g)2NO(g) H° = 181 kJ and S° = 24.9 J/K G°...

For the reaction N2(g) + O2(g)2NO(g) H° = 181 kJ and S° = 24.9 J/K G° would be negative at temperatures (above, below) K. Enter above or below in the first box and enter the temperature in the second box. Assume that H° and S° are constant.
A reaction has and △H°298 = 106 kJ/mol and △S°298 = 326 J /mol K at...

A reaction has and △H°298 = 106 kJ/mol and △S°298 = 326 J /mol K at 298 K. Calculate △G in kJ/mol.
For the reaction H^2 (g) + S(s) right arrow H^2 (g), delta?degree = - 20.2 kJ/mol...

For the reaction H^2 (g) + S(s) right arrow H^2 (g), delta?degree = - 20.2 kJ/mol and deltaSdegree = + 43.1 J/K-mol. Calculate deltaGdegree at 500degreeC. For the reaction H^2 (g) + S(s) right arrow H^2S(g), delta?degree = - 20.2 kJ/mol and deltaSdegree = + 43.1 J/K mol. Use the deltaGdegree value calculated at 500degreeC. Calculate deltaG for this reaction at 1500degreeC if P(H^2, g) = P(H^2S, g) = 10.0 atm. Show all standard calculation.

2. The reaction N2 (g)+3 F2 (g)2 NF3 (g), has AH° is -248.6 kJ mol and...

2. The reaction N2 (g)+3 F2 (g)2 NF3 (g), has AH° is -248.6 kJ mol and ArS° is -278.7J K mol. Calculate the temperature at which the reaction will be at equilibrium. Assume A,H° and A,S are independent of temperature.
For a given reaction, Delta H = -19.9 kJ/mol and Delta S = -55.5 J/K-mol. Calculate...

For a given reaction, Delta H = -19.9 kJ/mol and Delta S = -55.5 J/K-mol. Calculate the temperature in K where Delta G = 0. Assume that Delta H and Delta S do not vary with temperature. Also, what is the equilibrium constant at that temperature?
Given the following data: H3PO4(aq) H+ H2PO4-(aq) ∆Hof(kJ/mol) -1288.3 0 -1285 ∆S (J/mol.K ) 158.2 0...

Given the following data: H3PO4(aq) H+ H2PO4-(aq) ∆Hof(kJ/mol) -1288.3 0 -1285 ∆S (J/mol.K ) 158.2 0 89 (ΔGo = ΔHo -T ΔS; lnK = ΔGo/-RT) Calculate: 1. Standard free energy 2. K phosphoric acid and 3. Comment on the thermodynamic factors ( calculated ∆Ho and ∆S) that account/s for the fact that H3PO4 is a weak acid.

1)Consider the reaction B2H6(g) + 3 O2(g) → B2O3(s) + 3 H2O(g) ∆H = -2035 kJ/mol...

1)Consider the reaction B2H6(g) + 3 O2(g) → B2O3(s) + 3 H2O(g) ∆H = -2035 kJ/mol Calculate the amount of heat released when 37.1 g of diborane is burned. 2) Consider the reaction B2H6(g) + 3 O2(g) → B2O3(s) + 3 H2O(g) ∆H = -2035 kJ How much heat is released when a mixture of 9.71 g B2H6 and 1.53 g O2 is burned? 3)Consider the reaction B2H6(g) + 3 O2(g) → B2O3(s) + 3 H2O(g) ∆H = -2035 kJ...