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Hydrogen sulfide gas is a poisonous gas with the odor of rotten eggs. It occurs in natural gas and is produced during the decay of organic matter, which contains sulfur. The gas burns in oxygen as follows:

2H2S(g) + 3O2(g) → 2H2O(l) + 2SO2(g)

Calculate the standard enthalpy change for this reaction using standard enthalpies of formation.

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Related questions

Hydrogen sulfide, H2S, is a foul-smelling gas. It burns to form sulfur dioxide.

2H2S (g) + 3O2 (g) → 2SO2 (g) + 2H2O (g)                   ΔH = −1036 kJ

Calculate the enthalpy change to burn 27.4 g of hydrogen sulfide.

What is the balanced chemical equation for the reaction used to calculate ΔH∘f of CaCO3(s)? If fractional coefficients are required, enter them as a fraction (i.e. 1/3). Indicate the physical states using the abbreviation (s), (l), or (g) for solid, liquid, or gas, respectively without indicating allotropes. Use (aq) for aqueous solution. Express your answer as a chemical equation. The standard enthalpy of formation (ΔH∘f) is the enthalpy change that occurs when exactly 1 mol of a compound is formed from its constituent elements under standard conditions. The standard conditions are 1 atm pressure, a temperature of 25 ∘C , and all the species present at a concentration of 1 M . A "standard enthalpies of formation table" containing ΔH∘f values might look something like this: Substance ΔH∘f H(g) 218 kJ/mol H2(g) 0 kJ/mol Ca(s) 0 kJ/mol Ca2+(aq) −543 kJ/mol C(g) 71 kJ/mol C(s) 0 kJ/mol N(g) 473 kJ/mol O2(g) 0 kJ/mol O(g) 249 kJ/mol S2(g) 129 kJ/mol

The standard enthalpy of formation (ΔH∘f) is the enthalpy change that occurs when exactly 1 mol of a compound is formed from its constituent elements under standard conditions. The standard conditions are 1 atm pressure, a temperature of25 ∘C , and all the species present at a concentration of 1 M . A "standard enthalpies of formation table" containing ΔH∘f values might look something like this:
Substance ΔH∘f
H(g) 218 kJ/mol
H2(g) 0 kJ/mol
Ca(s) 0 kJ/mol
Ca2+(aq) −543 kJ/mol
C(g) 71 kJ/mol
C(s) 0 kJ/mol
N(g) 473 kJ/mol
O2(g) 0 kJ/mol
O(g) 249 kJ/mol
S2(g) 129 kJ/mol

Part A

What is the balanced chemical equation for the reaction used to calculate ΔH∘f of CaCO3(s)?

If fractional coefficients are required, enter them as a fraction (i.e. 1/3). Indicate the physical states using the abbreviation (s), (l), or (g) for solid, liquid, or gas, respectively without indicating allotropes. Use (aq) for aqueous solution.

Express your answer as a chemical equation.

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