(a) when 1/2N2(g)+3/2H2(g)?NH3(g) for NH3(g) find the value of ?H?f. (b) when S(s)+O2(g)?SO2(g) For SO2(g) find...

(a) when 1/2N2(g)+3/2H2(g)?NH3(g)

for NH3(g) find the value of ?H?f.

(b) when S(s)+O2(g)?SO2(g)

For SO2(g) find the value of ?H?f.

(c) when Rb(s)+12Cl2(g)+32O2(g)?RbClO3(s)

For RbClO3(s) find the value of ?H?f.

Expert Solution

The molar enthalpy of formation of a compound is the enthalpy change (heat) during the reaction of formation of 1 mole of the compound from its elements in their standard states (P=1 atm).

1 molecule of NH₃ contains 1 N atom and 3 H atoms. The standard states of N and H are N₂(g) and H₂(g), respectively.

The molar enthalpy of formation of NH₃ is the enthalpy change during the reaction of formation of 1 mole of NH₃ from N₂(g) and H₂(g).

1 molecule of SO₂ contains 1 sulfur atom and 2 oxygen atoms. The standard states of sulfur and oxygen are S(s) and O₂(g), respectively.

The molar enthalpy of formation of SO₂ is the enthalpy change during the reaction of formation of 1 mole of SO₂ from S(s) and O₂(g).

1 molecule of RbClO₃ contains 1 Rb atom, 1 Cl and 3 O atoms. The standard states of Rb and Cl, and O are Rb(s), Cl₂(g) and O₂(g), respectively.

The molar enthalpy of formation of RbClO₃ is the enthalpy change during the reaction of formation of 1 mole of RbClO₃from Rb(s), Cl₂(g) and O₂(g).

queen_honey_blossom answered 1 year ago

Consider the unbalanced reaction NiS2(s) + O2(g) --> NiO(s) + SO2(g). When 11.2g of NiS2 react...

Consider the unbalanced reaction NiS2(s) + O2(g) --> NiO(s) + SO2(g). When 11.2g of NiS2 react with 5.43g of O2, 4.86g of NiO are obtained. The theoretical yield of Nio is? The limiting reactant is? The percentage yield is what percent?

For the system SO3 ( g) ⇔ SO2 (g ) + 1 2 O2 ( g)...

For the system SO3 ( g) ⇔ SO2 (g ) + 1 2 O2 ( g) at 1000 K, K = 0.45. Sulfur trioxide, originally at 1.00 atm pressure, partially dissociates to SO2 and O2 at 1000 K. what is its partial pressure at equilibrium?

Which of the following processes is endothermic, given the following: S(s) + O2(g) → SO2(g) ΔH...

Which of the following processes is endothermic, given the following: S(s) + O2(g) → SO2(g) ΔH = –299 kJ/mol S(s) + 3/2 O2(g) → SO3(g) ΔH = –395 kJ/mol A) 2 S(s) + 2 O2(g) → 2 SO2(g) B) ½ S(s) + ½ O2(g) →½ SO2(g) C) 2 S(s) + 5/2 O2(g) → SO2(g) + SO3(g) D) SO3(g) → S(s) + 3/2 O2(g)

Consider the following system at equilibrium. S(s)+O2(g)<--->SO2(g) 1. How will adding more S(s) shift the equilibrium?...

Consider the following system at equilibrium. S(s)+O2(g)<--->SO2(g) 1. How will adding more S(s) shift the equilibrium? A) to the right B) to the left C) no effect 2. How will removing some SO2(g) shift the equilibrium? A) to the right B) to the left C) no effect 3. How will decreasing the volume of the container shift the equilibrium? A) to the right B) to the left C) no effect

1. ¬B∨(G↔J), H→(B&C) ∴(H&J)→G 2. A∨B, C↔¬(B∨D) ∴C→A 3. (A&B) ↔ (F→G), (A&F) & B∴(G→R)→R 4....

1. ¬B∨(G↔J), H→(B&C) ∴(H&J)→G 2. A∨B, C↔¬(B∨D) ∴C→A 3. (A&B) ↔ (F→G), (A&F) & B∴(G→R)→R 4. T→¬B, T→¬D ∴ T→¬(B∨D) 5. ¬(M∨¬S), S→(R→M) ∴A → (¬R∨T) 6. (F&G) → I, (I∨J) → K ∴F→(G→K) 7. ¬U, O→G, ¬(O∨G) →U ∴G Prove that the arguments are valid by constructing a dedication using the rules MP, MT, DN, Conj, Simp, CS, Disj, DS, DM, CP, HS, BE, and DL. Use CP if needed.

(a) Find ∆G◦ and K at 298.15 K for the gas-phase reaction 2 SO2(g) + O2(g)...

(a) Find ∆G◦ and K at 298.15 K for the gas-phase reaction 2 SO2(g) + O2(g) 2 SO3(g) (b) If a stoichiometric mixture of SO2 and O2 is allowed to come to equilibrium at 298.15 K and 1.000bar, find the partial pressure of SO2.

(a) (f ∘ g)(3) (b) g(f(2)) (c) g(f(5)) (d) (f ∘ g)(−3) (e) (g ∘ f)(−1) (f) f(g(−1))

1. Let g(s) = √ s. Find a simple function f so that f(g(s)) = 0....

1. Let g(s) = √ s. Find a simple function f so that f(g(s)) = 0. Hint: see Methods of computing square roots on Wikipedia. Use Newton’s method to estimate √ 2. Start with 3 different (and interesting) initial values of your choice and report the number of iterations it takes to obtain an accuracy of at least 4 digits. In python.

4 FeS2(s) + 11 O2(g) → 2 Fe2O3(s) + 8 SO2(g) ΔH = -3307.9 kJ 2...

4 FeS2(s) + 11 O2(g) → 2 Fe2O3(s) + 8 SO2(g) ΔH = -3307.9 kJ 2 H2S(g) + 3 O2(g) → 2 H2O(l) + 2 SO2(g) ΔH = -1125.2 kJ 4 FeO(s) + O2(g) → 2 Fe2O3(s) ΔH = 578.2 kJ 2 Fe(s) + O2(g) → 2 FeO(s) ΔH = -544 kJ H2(g) + S(s) → H2S(g) ΔH = -20.2 kJ 2 H2(g) + O2(g) → 2 H2O(l) ΔH = 571.7 kJ By combining the above equations calculate the ΔH(formation)...

Consider the combustion of acetamide: 4C2H5NO(s)+11O2(g)?8CO2(g)+10H2O(l)+2N2(g) ?H=?4738kJ Part A How much heat is released when 375.0 g...

Consider the combustion of acetamide: 4C2H5NO(s)+11O2(g)?8CO2(g)+10H2O(l)+2N2(g) ?H=?4738kJ Part A How much heat is released when 375.0 g of water is produced? Part B Acetamide has a density of 1.159 g/mL. What volume of acetamide must be combusted to result in the release of 1850 kJ of heat?

Question