Chemistry

Sulfur burns in oxygen in two steps:
i.S(s) + O2(g) ->SO2(g) change of Heat=-297kJ
ii. 2SO2(g) + O2(g)->2SO3(g) change of heat=-198kJ

Calculate the total heat released if this is the final reaction: 2S(s) + 3O2(g)->2SO3(g)

  1. 👍
  2. 👎
  3. 👁
  1. Hess' law. Multiply equation i by 2 (multiply H by 2 also) and add to equation ii. That will give you the equation you want so delta H for the final reaction is the sum of 2*i + ii = final rxn.

    1. 👍
    2. 👎

Respond to this Question

First Name

Your Response

Similar Questions

  1. Chemistry

    In the reaction 2H2S + 3O2 -> 2SO2 +2H2O, the oxidizing agent is 1.oxygen 2.water 3.sulfur dioxide 4.hydrogen sulfide oxygen?

  2. chemistry

    1. Chlorobenzene, C6H5Cl, is used in the production of chemicals such as aspirin and dyes. One way that chlorobenzene is prepared is by reacting benzene, C6H6, with chlorine gas according to the following BALANCED equation. C6H6

  3. Chemistry

    Elemental sulfur can be converted to sulfur dioxide by combustion in air. Sulfur dioxide will react with water to form sulfurous acid (see balanced equation below). SO2(g) + H2O(l) → H2SO3(l) What mass of sulfur dioxide is

  4. AP Chemistry

    For the system 2SO2(g) + O2(g) 2SO3 (g), change in enthalpy is negative for the production of SO3. At a particular temperature, 8.00 moles of sulfur dioxide and 10.00 moles of sulfur trioxide are introduced into a 2.00 L

  1. Chemistry

    Sulfur dioxide (SO2) is an unwelcome result of burning soft coal in power plants. Some of the SO2 ends up as sulfuric acid in acid precipitation. The net reaction is 2 SO2(g) + O2(g) + 2 H2O(ℓ) −→ 2 H2SO4(ℓ) What mass in

  2. Chemistry

    Sulfur trioxide decomposes into sulfur dioxide and oxygen in an equilibrium. You have a 3.00 L vessel that is charged with 0.755 mol of SO3. At equilibrium, the amount of SO3 is 0.250 mol. 2 SO3 (g) ----> 2 SO2 (g) +O2 (g) A)

  3. chemistry

    Use the thermochemical equations shown below to determine the enthalpy (kJ) for the reaction: H2SO3(l)=>H2S(g) + 3/2O2(g) H2SO3(l)=>H2O(l) +SO2(g) DH=62KJ SO2(g)=>S(s) + O2(g) DH=297KJ H2S(g) +1/2O2(g)=>S(s) + H2O(l) DH=-155KJ so

  4. Chemistry- please help ASAP!!!! thank you

    S(rhombic)+O2(g)--->SO2(g) change in H(rxn)= -296.06 kJ/mol S(monoclinic)+O2(g)--->SO2(g) change in H(rxn)= -296.36 kJ/mol 1. Calculate the enthalpy change for the transformation. S(rhombic)-->S(monoclinic) Our goal is to

  1. Chemistry

    Sulfur dioxide reacts with oxygen to form sulfur trioxide according to the equation 2SO2(g) + O2(g) 2SO3(g) Samples of sulfur dioxide, oxygen, and sulfur trioxide were added to a flask of volume 1.40 dm^3 and allowed to reach

  2. chemistry

    sulfur dioxide (g) + oxygen (g) sulfur trioxide (g) SO2 + O = SO3 Is this correct for the balanced equation?

  3. Chemistry

    Sulfur dioxide is used to make sulfuric acid. one method of producing it is by roasting mineral sulfides, for example, FeS2(s) + O2 (g) ---> SO2(g) + Fe2O3(s) (unbalanced). A production error leads to the sulfide being placed in a

  4. CHEMISTRY

    2H2S + 3O2 → 2H2O +2SO2 given the balanced equation, if 4 moles of hydrogen sulfide react: How many moles of oxygen consumed? How many moles of water and sulfur dioxide are produced?

You can view more similar questions or ask a new question.