The value of δs° for the oxidation of solid elemental sulfur to gaseous sulfur dioxide, s (s, rhombic) + o2 (g) → so2 (g) is j/k⋅mol. the value of s° for the oxidation of solid elemental sulfur to gaseous sulfur dioxide, s (s, rhombic) + o2 (g) so2 (g) is j/kmol. +248.5 +485.4 +11.6 -11.6 -248.5

Explanation:

You can calculate the entropy change of a reaction by using the standard molar entropies of reactants and products.

The formula is

The equation for the reaction is

                        S(s, rhombic) + O₂(g) ⟶ SO₂(g)

ΔS°/J·K⁻¹mol⁻¹         31.8            205.0      248.1

The difference probably arises for our use of different sources for the molar entropies.

first, consult an activity series chart to determine if al is more reactive than fe. it is, so it will replace the fe. now, one can continue with the problem.

next, make sure you have a correctly balanced equation.

3feo + 2al ==> 3fe + al2o3

now, determine which reactant (feo or al) is in limiting supply.

moles feo present = 125 g x 1 mole/71.8 g = 1.74 moles

moles al present = 25.0 g x 1 mole/26.98 g = 0.927 moles

since from the balanced equation, it take 3 mol feo for every 2 mol al, al will be limiting.

you can determine this simply by dividing moles of each by their coefficient in the balanced equation. for example: 1.74/3 = 0.58 and 0.927/2 = 0.464. al is less, so it is limiting.

finally, using the stoichiometry in the balanced eq. determine mass of fe that can be produced from 0.927 moles of al.

0.927 moles al x 3 moles fe/2 moles al x 55.8 g/mole = 77.6 g

answer; i believe the correct answer is (solid gold);