How much heat (in kilojoules) is evolved or absorbed in the reaction of 2.90g of Fe2O3 with enough carbon monoxide to produce iron metal?
Fe2O3 + 3CO ---> 2Fe + 3CO2 dH=-24.8kJ
How do you find q (of the 2Fe in kJ).
Pure substances have heat formation (delta Hf) of zero.
-24.8 kJ x (2.90g Fe2O3/molar mass Fe2O3) = -??
The minus sign means heat is evolved.
To find the heat evolved or absorbed in the reaction, you need to calculate the amount of heat produced or released per mole of Fe2O3 reacted.
1. Begin by calculating the molar mass of Fe2O3.
The molar mass of Fe2O3 is calculated as follows:
2(Fe) + 3(O) = 2(55.845 g/mol) + 3(16.00 g/mol) = 111.69 g/mol.
2. Determine the number of moles of Fe2O3 used.
Number of moles = mass (g) / molar mass (g/mol)
Number of moles = 2.90 g / 111.69 g/mol = 0.026 moles.
3. Since the reaction coefficient of Fe in the balanced equation is 2, the moles of Fe produced will be twice the moles of Fe2O3 used.
Number of moles of Fe = 2 * 0.026 moles = 0.052 moles.
4. Now, you can calculate the amount of heat (q) produced or absorbed in the reaction using the equation:
q = moles of substance * ΔH
q = 0.052 moles * (-24.8 kJ) = -1.2904 kJ
Therefore, the amount of heat evolved in the reaction of 2.90 g of Fe2O3 with enough carbon monoxide to produce iron metal is approximately -1.290 kJ.
Note: The negative sign indicates that the heat is evolved or released in the reaction.
To find the heat absorbed or evolved in the reaction of 2.90g of Fe2O3 with enough carbon monoxide to produce iron metal, you can use the equation:
q = m * ΔH
where:
q is the heat (in kJ)
m is the mass of Fe2O3 (in grams)
ΔH is the enthalpy change for the reaction (in kJ)
Given:
Mass of Fe2O3 (m) = 2.90g
Enthalpy change (ΔH) = -24.8 kJ
Now, let's plug in the values into the equation:
q = 2.90g * -24.8 kJ
To calculate q, multiply the mass of Fe2O3 by the enthalpy change:
q = -71.92 kJ
Therefore, the heat absorbed or evolved for the reaction of 2.90g of Fe2O3 is -71.92 kJ. Since the enthalpy change is negative, it means the reaction releases heat (exothermic).