Step 1: Explanation:
Note:
Step 2: write all the reactions
S(s) + 3/2 O2(g) ------------> SO3 (g) ΔG0 = -371 kJ -------> equation (1)
2SO2(g) + O2(g) ------------> 2SO3 (g) ΔG0 = -142 kJ -------> equation (2)
Our target equation is S(s) + O2(g) ------------> SO2 (g)
Step 3:
Now our target equation has no SO3, so we reverse equation 2 and multiply by 1/2 to cancel the SO3
1/2 × [ 2SO3 (g) ------------> 2SO2(g) + O2(g) ΔG0 = -142 kJ ]
SO3 (g) ------------> SO2(g) + 1/2O2(g) ΔG0 = +71 kJ -----> equation(3) [note: sign will reversed so it becomes +ve and value is also multiply by 1/2 so it becomes half of original value ]
Step 4:
Now add equation (1) and (3) and equation to get the target equation
S(s) + 3/2 O2(g) ------------> SO3 (g) ΔG0 = -371 kJ
SO3 (g) ------------> SO2(g) + 1/2O2(g) ΔG0 = +71 kJ
On adding the all the above equation we get
S(s) + 3/2 O2(g) + SO3 (g) -----------> SO3 (g) + SO2(g) + 1/2O2(g) ΔG0 = -371 kJ + ( 71 kJ ) = -300 kJ
Now, similar like species will cancel out ( here SO3 (g) , 1/2 O2(g) will cancel out ) from each side of reaction
So overall equation will becomes
S(s) + O2(g) -----------> SO2(g) ΔG0 = -300 kJ
(1) Hence ΔG0 of the reaction is -300 kJ
(2) yes the reaction is spontaneous
[ because if a reaction is exothermic the free energy change ( ΔG0 ) is negative and the reaction is always spontaneous.]
7 Coleulate Kt Given the following data: 4. (Equation 1) S(s) +3/202(g) - SO3(g) AG= -...
Given the following data: S(s) + 02(8) -> SO3(g) AH = -395.2 kJ 2SO2(g) + O2(g) + 2503(g) AH = - 198.2 kJ Calculate AH for the reaction: S(s) + O2(g) SO2(g) +296.1 kJ -494.3 kJ -296.1 kJ 0 -197.0 kJ -593.4 kJ
AG° = -300.1 kJ AG° =-742.1 kJ 4. Given that S(g) + O2(g) → SO2(g) 2S(g) + 302(g) → 2503(g) calculate AG of the following reaction: SO2(g) + 1/2O2(g) → SO3(g) a. –1042.2 kJ b. -71.0 kJ c. +2.47 kJ d. +71.0 kJ e. +1042.2 kJ
Given the following reactions: 2 S (s) + 3 O2 (g) ⟶ 2 SO3 (g) ΔH1= LaTeX: -− 790 kJ S (s) + O2 (g) ⟶ SO2 (g) ΔH2= LaTeX: -−297 kJ What is the enthalpy change of the following reaction? 2 SO3 (g) ⟶ 2 SO2 (g) + O2 (g) ΔH3=?
1). From the following enthalpy changes, S (s) + 3/2 O2 (g) → SO3 (9) 2 SO2 (g) + O2(g) → 2 SO3 (9) AH° = -395.2 kJ AH° = -198.2 kJ Calculate the value of AH° for the reaction by using Hess's law of Heat Summation S (s) + O2 (g) → SO2 (g).
s(s) + 3/2 O2 (g) = SO3 15. (6 pts) Given the data below, calculate the ΔΗ,xn for the reaction: AH -296.1 kJ S (s) + O2 (g) → SO2 (g) 2SOs (g)
Question 7 (1 point) Given the thermochemical equation O2(g)---> SO3(g) AH= -99.1 kJ/mol, S2(g) + calculate the enthalpy change when 89.6 g of SO2 is converted to SO3. -111 kJ 69.3 kJ O-69.3 kJ -139 kJ 139 kJ
Use the standard reaction enthalpies given below to determine ΔH°rxn for the following reaction: 4 SO3(g) → 4 S(s) + 6O2(g) ΔH°rxn = ? Given: SO2(g) → S(s) +O2(E) ΔH°rxn = +296.8 kJ 2 SO2(g) + O2(g) → 2SO3(g) ΔH°rxn = -197.8 kJ-494.6 kJ -692.4 kJ -791.4 kJ 1583 kJ 293.0 kJ
1).From the following enthalpy changes, S (s) +3/2 O2 (g) 2 SO2 (g) SO3 (g) O2 (g)2 SO3 (g) AH =-395.2 kJ AHo 198.2 kJ Calculate the value of AHo for the reaction by using Hess's law of Heat Summation S(s) O2 (g) SO2 (g) 2) Oxyacetylene torches are fueled by the combustion of acetylene, C2H2. 4 CO2 (g) +2 H20 (g) 2 C2H2 + 5 O2 (g) If the enthalpy change for the reaction is -2511.14 kJ/mol, a) How...
IS LOCAS Question 16 5 pts Given the following data: S(s) + O2(g) → SO3(8) AH=-395.2 kJ 2502(g) + O2(g) - 2503(g) AH = - 198.2 kJ Calculate AH for the reaction: S(s) + O2(g) +SO2(g) -197.0 kJ 0 -593.4 kJ -296.1 kJ -494.3 kJ +296.1 kJ 5 pts Question 17
Use the given K’s below determine Ktot for the following reaction: 4 SO3(g) → 4 S(s) + 6 O2(g) Ktot = ? Given: SO2(g) → S(s) + O2(g) K1 = 2.9 x 10-3 2 SO2(g) + O2(g) → 2 SO3(g) K2 = 7.5 x 104