hydrogen sulfide gas, H2S(g)H2S(g), reacts with oxygen gas, O2(g)O2(g) , sulfur dioxide gas, SO2(g)SO2(g), and steam, H2O(g)H2O(g), are produced. This is given by: 2H2S(g)+3O2(g)→2H2O(g)+2SO2(g) Use the table of standard enthalpies of formation to calculate the standard change in enthalpy of the given reaction

2. In studying the energy generated by a person, you may view the person roughly as a constant pressur calorimeter using sugar (i.e., sucrose, C₁2H₂2O11) to generate power. The reaction of table sugar in calorimeter is given by + Ch. 9 Sl....pdf C12H22O11(s)+120₂(g) →12CO₂(g)+11H₂O+heat. C. a. What is the heat released by consuming one mole of sugar (C₁2H22O11) in this b. Calculate the enthalpy of combustion per sugar utilization. mole Does the result of your calculation make I wi (540 Karak 14 11 M de 2009 1 AP fik Tour of 1 way? 20

If the following three thermochemical equations are added together, what is the resulting equation:2 XO2 (g) +2 CO (g) →→ 2 XO (g) + 2 CO2 (g)2 XO (g) + 2/3 CO2(g) →→ 2/3 X3O4 (s) + 2/3 CO (g)2/3 X3O4 (s) + 1/3 CO2 (g) →→ X2O3 (g) + 1/3 CO (g)     Question 17 options:   6 XO (g) + 2 CO2(g) →→ 2 X3O4 (s) + 2 CO (g)   2 XO2 (s) + CO (g) →→ X2O3 (s) + CO2 (g)   C (s) + 3 XO2 (g) →→ X3O4 (g) + CO2 (g)   2 X3O4 (s) + CO2 (g)  →→ 3 X2O3 (g) + CO (g)   CO (g) + XO2 (g) →→ XO (g) + CO2 (g)

Calculate how much heat is released when 100. Grams of NO is mixed with 75 grams of O2.2NO(g) + O2(g)→ 2NO2(g) ?H= - 116kJ5. What is the limiting reagent

and 2 Enthalpy #1.30 enoindice pled TT 2010 2D49.bs 22) When 1 mole of Fe2O3(s) reacts with H₂(g) to form Fe(s) and H2O(g) according to the following equation, 98.8 kJ of energy are absorbed. (6 Fe2O3(s) + 3 H2(g) → 2 Fe(s) + 3 H₂O(g) (pp) (20/d4 (pm) $40 D Reaclanis 13:48 SH Products endothermic, A endothermic, B (2) exothermic, A exothermic, B nad W (21 Enthalpy MOMS. Reactants Products (A) (B) Is the reaction endothermic or exothermic, and which of the enthalpy diagrams above represents grow olor and to noin (01 this reaction? SH GH TH A HOMH X HILD 08.10 Page 6 of 8

Use the given equations to determine the enthalpy, ΔHrxn, per mole of reaction for the chemical equation below. Report your answer to one decimal place and do not include units.  P4(s) + 6H2(g) + 6O2(g) → 4H3PO3(aq)

In the following equation for a chemical reaction, the notation (s), (1), or (g) indicates whether the substance indicated is in the solid, liquid, or gaseous state. 2NO(g) + 2H2(g) →N2(g) + 2H,O(M) + energy Identify each of the following as a product or a reactant: H2O)| NO(g) N2(g) H2(g) When the reaction takes place energy is The reaction is

Ery 1 3 M (M) 2req The production capacity for acrylonitrile (C3H3N) in the United States is over 2 billion pounds per year. Acrylonitrile, the building block for polyacrylonitrile fibers and a variety of plastics, is produced from gaseous propylene, ammonia, and oxygen: 2C3H6(g) + 2NH3(g) + 30₂(g) → 2C3H3N(g) + 6H₂O(g) Assuming 100% yield, determine the mass of acrylonitrile which can be produced from the mixture below: Mass 7.28x102 g 5.00 x 102 g 1.00 x 103 g In progress Reactant oxygen propylene ammonia oxygen What mass of water is formed from your mixture? mass of water formed = g Calculate the mass (in grams) of each reactant after the reaction is complete: Submit g = mass of acrylonitrile produced Reactant Mass remaining propylene ammonia Show Hints ס ס ס g g Cengage Learning Cengage Technical Support Previous Next Save and Exit

Express the quantity in the unit indicated and designate whether this heat is gained or lost by the substance a. The quantity of heat in calories when 162.5 grams of water undergoes a temperature decrease from 45.84 C to 40.00 C. b. The quantity of heat in Kilojoules when 43.5 Kg of chloroform ,CHCl3 has its temperature changed from 16.8 C to 22.3 C ( sp ht of CHCl3 = 0.971 KJ/kg- C)

An industrial process for manufacturing sulfuric acid, H2SO4, uses hydrogen sulfide, H2S, from the purification of natural gas.  In the first step of this process, the hydrogen sulfide is burned to obtain sulfur dioxide, SO2. 2H2S(g) + 3 O2(g) → 2 H2O(l) + 2 SO2(g); ∆H = -1124 kJ.  The density of sulfur dioxide at 25 °C and 1.00 atm is 2.62 g/L, and the molar heat capacity is 30.2 J/mol °C. a) How much heat would be evolved in producing 1.00 L of SO2 at 25 °C and 1.00 atm?  b) Suppose heat from this reaction is used to heat 1.00 L of SO2 from 25 °C to 500 °C for its use in the next step of the process.  What percentage of the heat evolved is required for this?