Question

In: Chemistry

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) of FeS2(s).

Solutions

Expert Solution

Calculations are uploaded as images.

queen_honey_blossom answered 2 years ago
Next > < Previous

Related Solutions

Sulfuric acid is produced by the following process:     FeS2 + O2 →    Fe2O3 +   SO2...
Sulfuric acid is produced by the following process:     FeS2 + O2 →    Fe2O3 +   SO2    SO2 + O2 →    SO3    SO3 + H2O → H2SO4 Balance each reaction and then write a balanced net reaction. How many moles of O2 and H2O will be needed when 10.0 kg of FeS2 reacts completely?
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)
Given the data N2(g) + O2(g) → 2 NO(g) ΔH = +180.7 kJ 2 NO(g) +...
Given the data N2(g) + O2(g) → 2 NO(g) ΔH = +180.7 kJ 2 NO(g) + O2(g) → 2 NO2(g) ΔH = −113.1 kJ 2 N2O(g) → 2 N2(g) + O2(g) ΔH = −163.2 kJ use Hess's law to calculate ΔH for the reaction N2O(g) + NO2(g) → 3 NO(g).
Calculate the enthalpy change for the reaction: 4 Fe(s) + 3 O2(g) → 2 Fe2O3(s)     ...
Calculate the enthalpy change for the reaction: 4 Fe(s) + 3 O2(g) → 2 Fe2O3(s)            ΔH°rxn = ? where: 2 Fe(s) + 6 H2O(ℓ) → 2 Fe(OH)3(s) + 3 H2(g)               ΔH1° = +321.8 kJ                     2 H2O(ℓ) → 2 H2(g) + O2(g)                               ΔH2° = +571.7 kJ Fe2O3(s) + 3 H2O(ℓ) → 2 Fe(OH)3(s)                                 ΔH3° = +288.6 kJ
S(s,rhombic) + 2CO(g) ------> SO2(g) + 2C(s,graphite) ΔH° = -75.8 kJ and ΔS° = -167.6 J/K...
S(s,rhombic) + 2CO(g) ------> SO2(g) + 2C(s,graphite) ΔH° = -75.8 kJ and ΔS° = -167.6 J/K The maximum amount of work that could be done when 1.81 moles of S(s,rhombic) react at 323 K, 1 atm is _______ kJ. Assume that ΔH° and ΔS° are independent of temperature. Please answer it kJ
Given the following thermochemistry equations: C(s) + 1/2 O2(g) -------> CO (g); ΔH = -110.4 kJ/mol...
Given the following thermochemistry equations: C(s) + 1/2 O2(g) -------> CO (g); ΔH = -110.4 kJ/mol H2 (g) + 1/2 O2 (g) ------> H2O (l); ΔH = -285.5 kJ/mol CO(g) + 1/2 O2(g) -------> CO2 (g); ΔH = -283.0 kJ/mol HCOOH (l) + 1/2 O2 (g) ------> H2O (l) + CO2(g); Δ = -259.6 kJ/mol a) Calculate the ΔH for the formation of HCOOH. b) Calculate the ΔH of the reaction if 0.76 mL of HCOOH is obtained. c) If...
Calculate ΔHrxn for the following reaction: Fe2O3(s)+3CO(g)→2Fe(s)+3CO2(g) Use the following reactions and given ΔH′s. 2Fe(s)+3/2O2(g)→Fe2O3(s), ΔH...
Calculate ΔHrxn for the following reaction: Fe2O3(s)+3CO(g)→2Fe(s)+3CO2(g) Use the following reactions and given ΔH′s. 2Fe(s)+3/2O2(g)→Fe2O3(s), ΔH = -824.2 kJ CO(g)+1/2O2(g)→CO2(g), ΔH = -282.7 kJ
Calculate ΔHrxn for the following reaction: Fe2O3(s)+3CO(g)→2Fe(s)+3CO2(g) Use the following reactions and given ΔH′s. 2Fe(s)+3/2O2(g)→Fe2O3(s), ΔH...
Calculate ΔHrxn for the following reaction: Fe2O3(s)+3CO(g)→2Fe(s)+3CO2(g) Use the following reactions and given ΔH′s. 2Fe(s)+3/2O2(g)→Fe2O3(s), ΔH = -824.2 kJ CO(g)+1/2O2(g)→CO2(g), ΔH = -282.7 kJ
Calculate ΔHrxn for the following reaction: Fe2O3(s)+3CO(g)→2Fe(s)+3CO2(g) Use the following reactions and given ΔH′s. 2Fe(s)+3/2O2(g)→Fe2O3(s), ΔH...
Calculate ΔHrxn for the following reaction: Fe2O3(s)+3CO(g)→2Fe(s)+3CO2(g) Use the following reactions and given ΔH′s. 2Fe(s)+3/2O2(g)→Fe2O3(s), ΔH = -824.2 kJ CO(g)+1/2O2(g)→CO2(g), ΔH = -282.7 kJ
1.) Given the following data: C2H2(g) + 5/2 O2(g) à2CO2(g) + H2O(l)      ΔH= -1300.kJ C(s) +...
1.) Given the following data: C2H2(g) + 5/2 O2(g) à2CO2(g) + H2O(l)      ΔH= -1300.kJ C(s) + O2(g) àCO2(g)                                   ΔH= -394kJ H2(g) + O2(g) à H2O(l)                                 ΔH= -286kJ Use Hess’s Law to calculate ΔH for the reaction 2C(s) + H2(g) àC2H2(g) 2.) Calculate ΔH° for each of the following reactions using the data for the enthalpy of formation in the appendix. 2Na(s) + 2H2O(l)à2NaOH(aq) + H2(g
ADVERTISEMENT
Subjects
ADVERTISEMENT
Latest Questions
ADVERTISEMENT