Use the values found in Thermodynamic Properties to determine ΔS°, ΔH° and ΔG° at 298 K...

Use the values found in Thermodynamic Properties to determine ΔS°, ΔH° and ΔG° at 298 K for the reaction below. Enter all values to the 0.1 place.

4 NH3(g) + 5 O2(g) → 4 NO(g) + 6 H2O(g)

ΔS°

ΔH°

ΔG°

Expert Solution

4 NH3(g) + 5 O2(g) ----------------> 4 NO(g) + 6 H2O(g)

Hrxn = Hproducts - Hreactants

= ( 4 x 90.25 + 6 x -241.8 ) - (4 x –46.11+0 )

= - 905.36 kJ /mol

Srxn = Sproducts - Sreactants

= (4 x 210.6 + 6 x 188.7 ) - ( 4 x 192.3 + 5 x 205)

= 180.4 J / mol K

Grxn = Gproducts - Greactants

= (4 x 86.57 + 6 x –228.6 ) - ( 4 x –16.48 + 0 )

= - 959.4 kJ / mol

queen_honey_blossom answered 2 years ago

Consider a reaction with the following thermodynamic properties. ΔH° = 77.7 kJ ΔS° = –35.7 J/(K...

Consider a reaction with the following thermodynamic properties. ΔH° = 77.7 kJ ΔS° = –35.7 J/(K • mol) ΔG°= 88.4 kJ This reaction: will proceed very slowly. will be spontaneous at low temperatures. has bonds in the products that are weaker than the reactants. may have fewer and more complicated molecules in the product.

Given the values of ΔH∘rxn, ΔS∘rxn, and Tbelow, determine ΔSuniv. A. ΔH∘rxn=− 118 kJ , ΔS∘rxn=...

Given the values of ΔH∘rxn, ΔS∘rxn, and Tbelow, determine ΔSuniv. A. ΔH∘rxn=− 118 kJ , ΔS∘rxn= 258 J/K , T= 294 K B. ΔH∘rxn= 118 kJ , ΔS∘rxn=− 258 J/K , T= 294 K C. ΔH∘rxn=− 118 kJ , ΔS∘rxn=− 258 J/K , T= 294 K . D. ΔH∘rxn=− 118 kJ , ΔS∘rxn=− 258 J/K , T= 545 K . Predict whether or not the reaction in part A will be spontaneous. Predict whether or not the reaction in part...

Given the values of ΔH∘rxn , ΔS∘rxn , and T below, determine ΔSuniv . a) ΔH∘rxn=...

Given the values of ΔH∘rxn , ΔS∘rxn , and T below, determine ΔSuniv . a) ΔH∘rxn= 87 kJ , ΔSrxn= 146 J/K , T= 296 K Will this be spontaneous or not spontaneous? b) ΔH∘rxn= 87 kJ , ΔSrxn= 146 J/K , T= 762 K Will this be spontaeous or not spontaneous? c) ΔH∘rxn= 87 kJ , ΔSrxn=− 146 J/K , T= 296 K will this be spontaneous or not spontaneous? d) ΔH∘rxn=− 87 kJ , ΔSrxn= 146 J/K ,...

Calculate the value of ΔG°, ΔH°, & ΔS° for the formation of phosphorous trichloride from its...

Calculate the value of ΔG°, ΔH°, & ΔS° for the formation of phosphorous trichloride from its constituent elements at 25°C. P2 (g) + 3Cl2 (g) → 2PCl3 (g) is ________ kJ/mol.

Use data from Appendix C to calculate the equilibrium constant, K, and ΔG∘ at 298 K...

Use data from Appendix C to calculate the equilibrium constant, K, and ΔG∘ at 298 K for each of the following reactions. H2(g)+I2(g)⇌2HI(g) Calculate ΔG∘. Express your answer to four significant figures and include the appropriate units. Part A H2(g)+I2(g)⇌2HI(g) Calculate ΔG∘. Express your answer to four significant figures and include the appropriate units. Part B Calculate the equilibrium constant, K. Express your answer using two significant figures. Part C C2H5OH(g)⇌C2H4(g)+H2O(g) Calculate ΔG∘. Express your answer to two significant figures...

Given the values of ΔH∘rxn, ΔS∘rxn, and T below, determine ΔSuniv. Predict whether or not each...

Given the values of ΔH∘rxn, ΔS∘rxn, and T below, determine ΔSuniv. Predict whether or not each reaction will be spontaneous. ΔH∘rxn=− 118 kJ , ΔS∘rxn= 261 J/K , T= 294 K ΔSuniv = ??? (J/K) ΔH∘rxn= 118 kJ , ΔS∘rxn=− 261 J/K , T= 294 K . ΔSuniv = ??? (J/K) ΔH∘rxn=− 118 kJ , ΔS∘rxn=− 261 J/K , T= 294 K . ΔSuniv = ??? (J/K) ΔH∘rxn=− 118 kJ , ΔS∘rxn=− 261 J/K , T= 565 K . ΔSuniv...

For the reaction 2SO2(g) + O2(g) → 2SO3(g), ΔH° and ΔS° are both negative at 298...

For the reaction 2SO2(g) + O2(g) → 2SO3(g), ΔH° and ΔS° are both negative at 298 K, and the process is spontaneous at 298 K. Which of the following statements must also be true? A.ΔG is positive for the reaction at 298 K. B.The change in entropy is the driving force of the reaction. C.ΔG is temperature independent. D.The direction of the reaction may be reversed at high temperatures. E.At high temperature, ΔH becomes positive.

Use ΔGº =ΔHº -TΔSº to calculate ΔG (in kJ) at 298 K for : 2CO2(g) +4H2O(l)...

Use ΔGº =ΔHº -TΔSº to calculate ΔG (in kJ) at 298 K for : 2CO2(g) +4H2O(l) → 2CH3OH(l) + 3O2(g) If the above reaction could be done at 2081 K, what would be your estimate for ΔGº (in kJ) at this elevated temperature? Use ΔGº =ΔHº -TΔSº and assume ΔHº and ΔSº are independent of temperature. (The º is included because it is still for standard conditions, that is, 1 atm for gases and 1 molar for concentrations.)

For each of the following reactions, calculate ΔH∘rxn, ΔS∘rxn, and ΔG∘rxn at 25 ∘C. State whether...

For each of the following reactions, calculate ΔH∘rxn, ΔS∘rxn, and ΔG∘rxn at 25 ∘C. State whether or not the reaction is spontaneous. If the reaction is not spontaneous, would a change in temperature make it spontaneous? If so, should the temperature be raised or lowered from 25 ∘C?2CH4(g)→C2H6(g)+H2(g), Calculate ΔS∘rxn at 25 ∘C. 2NH3(g)→N2H4(g)+H2(g) Calculate ΔS∘rxn at 25 ∘C. N2(g)+O2(g)→2NO(g) Calculate ΔS∘rxn at 25 ∘C. 2KClO3(s)→2KCl(s)+3O2(g) Calculate ΔS∘rxn at 25 ∘C.

For each of the following reactions, calculate ΔH∘rxn, ΔS∘rxn, ΔG∘rxn at 25 ∘C. State whether or...

For each of the following reactions, calculate ΔH∘rxn, ΔS∘rxn, ΔG∘rxn at 25 ∘C. State whether or not the reaction is spontaneous. If the reaction is not spontaneous, would a change in temperature make it spontaneous? If so, should the temperature be raised or lowered from 25 ∘C? a) 2CH4(g)→C2H6(g)+H2(g) b) 2NH3(g)→N2H4(g)+H2(g) c) N2(g)+O2(g)→2NO(g) d) 2KClO3(s)→2KCl(s)+3O2(g) Can you please show equations. I am having so much trouble with these.

Question