Question

Calculate d r h0 for the following reaction at 25°c : fe3o4(s) co(g) ___→ 3feo(s) CO₂⁺(g) dhf o (kj/mol) –1118 –110.5 –272 –393.5?

Answer 1

To calculate the mass of CO required to react with Fe₂O3, first balance the equation, calculate the molar mass of Fe₂O3 and CO, and use conversion factors to find the mass of CO required.

Step-by-step explanation:

To calculate the mass of CO required to react with 25.13 g of Fe₂O3, we first need to balance the equation:

Fe₂O3 + 3CO → 2Fe + 3CO₂

Next, we need to calculate the molar mass of Fe₂O3 and CO. The molar mass of Fe₂O3 is 159.69 g/mol, and the molar mass of CO is 28.01 g/mol. Using the molar mass of CO, we can set up a conversion factor:

1 mol CO = 28.01 g CO

We can use this conversion factor to calculate the moles of CO required:

25.13 g Fe₂O3 * (1 mol Fe₂O3 / 159.69 g Fe₂O3) * (3 mol CO / 1 mol Fe₂O3) * (28.01 g CO / 1 mol CO) = 52.57 g CO

Therefore, 52.57 g of CO is required to react with 25.13 g of Fe₂O3.

Answer 2

The reaction given is
`\(Fe_3O_4(s) + 4CO(g) \rightarrow 3FeO(s) + 4CO_2(g)\)`. The change in enthalpy
`(\(\Delta H_0\))` for the reaction is calculated as
`\(\Delta H_0 = \sum n\Delta H_f^0(\text{products}) - \sum m\Delta H_f^0(\text{reactants})\)`, where n and m are the coefficients in the balanced equation. Substituting the given values, the reaction enthalpy
`(\(\Delta H_0\)) is \(+16.5 \, \text{kJ/mol}\).`

Step-by-step explanation:

The enthalpy change
`(\(\Delta H_0\))` for the reaction is determined by summing the standard enthalpies of formation
`(\(\Delta H_f^0\))` for the products and subtracting the sum of the
`\(\Delta H_f^0\)` values for the reactants. The given reaction is
`\(Fe_3O_4(s) + 4CO(g) \rightarrow 3FeO(s) + 4CO_2(g)\)`. Using the standard enthalpies of formation provided, we substitute the values into the formula
`\(\Delta H_0 = \sum n\Delta H_f^0(\text{products}) - \sum m\Delta H_f^0(\text{reactants})\)`. After calculations, the result is
`\(+16.5 \, \text{kJ/mol}\),` indicating that the reaction is endothermic.

In this context, the positive sign of
`\(\Delta H_0\)` implies that the reaction absorbs heat from the surroundings. The reactants have lower enthalpy than the products, and as a result, the reaction requires an input of energy. Understanding the sign of
`\(\Delta H_0\)` is crucial for predicting whether a reaction is exothermic or endothermic and helps in assessing the heat flow associated with the chemical transformation.