Question

find the amount of energy needed to break down rust, iron (III) oxide, Fe2O3(s), to form 50.0 g of oxygen gas. Given: the molar mass of iron and oxygen is 55.85 g/mol and 16.00 g/mol respectively; and the enthalpy of formation of Fe2O3 is -824.2 kJ/mol.

Answer 1

To find the amount of energy needed to break down rust, iron (III) oxide, Fe2O3(s), to form 50.0 g of oxygen gas, use stoichiometry and mole ratios. Convert the given mass of oxygen gas to moles and determine the ratio of Fe2O3 to O2 using a balanced chemical equation.

Step-by-step explanation:

The amount of energy needed to break down rust, iron (III) oxide, Fe2O3(s), to form 50.0 g of oxygen gas can be calculated using the enthalpy of formation of Fe2O3. To find the energy, we can use the concept of stoichiometry and mole ratios. First, convert the given mass of oxygen gas to moles. Then, use the balanced chemical equation to determine the ratio of Fe2O3 to O2. Finally, multiply the number of moles of Fe2O3 by the enthalpy of formation of Fe2O3 to find the amount of energy.

energy needed to break down rust, iron (III) oxide, Fe2O3(s), to form 50.0 g of oxygen gas, use stoichiometry and mole ratios. Convert the given mass of oxygen gas to moles and determine the ratio of Fe2O3 to O2 using a balanced chemical equation. Multiply the number of moles of Fe2O3 by the enthalpy of formation of Fe2O3 to find the energy.