Consider the following reaction at 298 K: 4Al(s) + 3O2(g) ==> 2Al2O3(s) Delta H= -3351.4 kJ/mol...

Consider the following reaction at 298 K: 4Al(s) + 3O2(g) ==> 2Al2O3(s)
Delta H= -3351.4 kJ/mol

Calculate:

a. Delta Ssystem = _______J/mol*K

b. Delta Ssurroundings = _______J/mol*K

c. Delta S universe = _________J/mol*K

Expert Solution

delta Sf (AL2O3) = 50.92 J/molK
delta Sf (O2) = 205.14 J/molK
delta Sf (Al) = 28.33 J/molK

Reaction taking place is:
4Al +3 O2 --->2Al2O3
a.
delts S sys = delta Sf (products) - delta Sf (reactsnta)
                      = 2*delta Sf (Al2O3) - 4* delta Sf (Al) - 3*delta Sf (O2)
                      = 2*(50.92) - 4*(28.33) -3*(205.14)
                       = -626.9 J/molK
b.
q sys= delta H = -3351.4 KJ/mol = -3351400 J/mol
q surr = -qsys = 3351400 J/mol
I am assuming tempearture os 298 K
delta S surrounding = qsurr/T
                                           =3351400/298
                                            = 11246.3 J/molK

c.
delta S univ = delta S sys +delta S surr
= -626.9 +11246.31
= 10619.4 J/molK

queen_honey_blossom answered 1 year ago

A reaction has and △H°298 = 151 kJ/mol and △S°298 = 286 J /mol K at...

A reaction has and △H°298 = 151 kJ/mol and △S°298 = 286 J /mol K at 298 K. Calculate △G in kJ/mol.

Consider the following reaction at 298 K: C(graphite)+2CL(g)------> CCl4(l) delta H=-139 kj Calculate delta S sys...

Consider the following reaction at 298 K: C(graphite)+2CL(g)------> CCl4(l) delta H=-139 kj Calculate delta S sys delta S surr delta S univ

Oxygen gas reacts with powdered aluminum according to the following reaction: 4Al(s)+3O2(g)→2Al2O3(s)..What volume of O2 gas...

Oxygen gas reacts with powdered aluminum according to the following reaction: 4Al(s)+3O2(g)→2Al2O3(s)..What volume of O2 gas (in L), measured at 795 mmHg and 16 ∘C, is required to completely react with 53.3 g of Al?

Consider the reaction: 2 NO2(g) → N2O4(g) Calculate ΔG (in kJ/mol) at 298°K if the equilibrium...

Consider the reaction: 2 NO2(g) → N2O4(g) Calculate ΔG (in kJ/mol) at 298°K if the equilibrium partial pressures of NO2 and N2O4 are 1.337 atm and 0.657 atm, respectively.

Consider this reaction: 2CH3OH(l) + 3O2(g)2O(l) + 2CO2(g) H = –1452.8 kJ/mol a.Is this reaction endothermic...

Consider this reaction: 2CH3OH(l) + 3O2(g)2O(l) + 2CO2(g) H = –1452.8 kJ/mol a.Is this reaction endothermic or exothermic? b.H if the equation is multiplied throughout by 2? c.H if the direction of the reaction is reversed so that the products become the reactants and vice versa? What is the value of ∆H if water vapor instead of liquid water is formed as the product?

The following equation shows the conversion of aluminum oxide (from the ore bauxite) to aluminum: 2Al2O3(s)→4Al(s)+3O2(g),...

The following equation shows the conversion of aluminum oxide (from the ore bauxite) to aluminum: 2Al2O3(s)→4Al(s)+3O2(g), ΔH = +801 kcal (+3350 kJ ) Part B: How many kilocalories are required to produce 1.16 mol of aluminum? Part C: How many kilojoules are required to produce 1.16 mol of aluminum? Part D: How many kilocalories are required to produce 11.6 g of aluminum? Part E: How many kilojoules are required to produce 11.6 g of aluminum?

Consider this reaction: 2O3(g)<--->3O2(g) ΔHrxn=-285.4 kj/mol. In which direction will the reaction shift when the following...

Consider this reaction: 2O3(g)<--->3O2(g) ΔHrxn=-285.4 kj/mol. In which direction will the reaction shift when the following stresses are combined? a.Remove ozone from the system b.Add Ar c.Decrease temperature d.Add catalyst

Part 1. Consider the following reaction at 298 K: 2H2(g)+O2(g)---->2H2O(g) ΔH=-483.6 kj/mol Calculate the following quantities:...

Part 1. Consider the following reaction at 298 K: 2H2(g)+O2(g)---->2H2O(g) ΔH=-483.6 kj/mol Calculate the following quantities: ΔSsys=____J(molxK) ΔSsurr=____J(molxK) ΔSuniv=____J (molxK) Part 2. For a particular reaction, ΔH = 168.1 kJ/mol and ΔS = -55.8 J/(mol·K). Calculate ΔG for this reaction at 298 K. Is this system spontaneaus as written, Is it in the reverse direction, Or is it at equilibrium?

1. Consider the following thermochemical equation: 2ZnS(s) + 3O2(g) → 2ZnO(s) + 2SO2(g) ∆H° = –878.2 kJ

1. Consider the following thermochemical equation: 2ZnS(s) + 3O2(g) → 2ZnO(s) + 2SO2(g) ∆H° = –878.2 kJ (a) How much heat is released when 3.0 mol ZnS(s) reacts in excess oxygen? (b) How much heat is released when 2.3 × 10-2 mol ZnS(s) reacts in excess oxygen? (c) What is the enthalpy change when 223.9 g ZnS(s) reacts in excess oxygen? (d) What is the enthalpy change when 0.96 g ZnO(s) is produced? 2. Slaked lime (Ca(OH)2(s)) is produced...

1. A chemical reaction at 304 K has an enthalpy change (delta-H) of -73.9 kJ/mol and...

1. A chemical reaction at 304 K has an enthalpy change (delta-H) of -73.9 kJ/mol and an entropy change (delta-S) of 161.6 kJ/mol. What is its Gibbs energy change, delta-G, in kJ/mol? Give the answer to one decimal place. 2.Use the thermodynamic data in your textbook to determine the temperature below which the following reaction is spontaneous. (Give the temperature in K, to the nearest degree.) 2SO2 (g) + O2 (g) -- 2SO3 (g) 3.What is the delta-G for the...

Question