Question

При соединении 28 грамм железа с серой выделилось 48.8 кДж теплоты .Вычислите тепловой эффект реакции образования сульфида железа(II)???

Answer 1

Fe+S=FeS+Q
v(Fe)=28/56=0.5 моль
=> Q=48.8*2=97.6

Answer 2

Calculation of the Heat Effect of the Formation of Iron(II) Sulfide

To calculate the heat effect of the formation of iron(II) sulfide, we need to use the law of conservation of energy, which states that energy cannot be created or destroyed, only transferred or converted from one form to another. In this case, the heat released during the reaction is equal to the heat absorbed or released during the formation of the product.

The given information states that when 28 grams of iron is combined with sulfur, 48.8 kJ of heat is released. We can use this information to calculate the heat effect of the formation of iron(II) sulfide.

The balanced chemical equation for the formation of iron(II) sulfide is:

Fe + S → FeS

From the equation, we can see that 1 mole of iron reacts with 1 mole of sulfur to form 1 mole of iron(II) sulfide.

To calculate the heat effect, we need to convert the mass of iron to moles. The molar mass of iron is 55.845 g/mol, so:

Number of moles of iron = mass of iron / molar mass of iron

Number of moles of iron = 28 g / 55.845 g/mol

Now, we can use the stoichiometry of the balanced equation to relate the moles of iron to the moles of iron(II) sulfide. Since the stoichiometric coefficient of iron in the balanced equation is 1, the number of moles of iron(II) sulfide formed will also be 1.

Finally, we can calculate the heat effect of the reaction using the equation:

Heat effect = heat released / moles of iron(II) sulfide formed

Heat effect = 48.8 kJ / 1 mol

Therefore, the heat effect of the formation of iron(II) sulfide is 48.8 kJ/mol.

Please note that the provided sources did not contain any relevant information for this specific calculation.