Question

What mass of iron must be in a hot pack to provide -335 kJ of heat when the iron reacts with oxygen and is converted to iron (III) oxide according to the following equation? 2 Fe (s) + 1.5 O2 (g) → Fe2O3 (s) ∆H° = -824.2 kJ/mol.

Name: what mass of iron must be in a hot pack to provide 335 kj of heat when the iron reacts with oxygen and is converted to iron iii oxide according to the following equation 2 fe s 15 o2 g fe2o3 03334
Uploaded: 2021-10-07T17:44:55-08:00
Duration: 3 min 16 s
Channel: Jennifer Hudspeth
Description: what mass of iron must be in a hot pack to provide 335 kj of heat when the iron reacts with oxygen and is converted to iron iii oxide according to the following equation 2 fe s 15 o2 g fe2o3 03334

          What mass of iron must be in a hot pack to provide -335 kJ of heat when the iron reacts with oxygen and is converted to iron (III) oxide according to the following equation? 2 Fe (s) + 1.5 O2 (g) → Fe2O3 (s) ∆H° = -824.2 kJ/mol.

Added by Andrew D.

Chemistry: Structure and Properties

Nivaldo Tro 2nd Edition

Instant Answer

Solved by Expert Jennifer Hudspeth

10/07/2021

Step 1

Given: ΔH° = -824.2 kJ/mol -335 kJ ÷ -824.2 kJ/mol = 0.407 mol Fe2O3 Show more…

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What mass of iron must be in a hot pack to provide -335 kJ of heat when the iron reacts with oxygen and is converted to iron (III) oxide according to the following equation? 2 Fe (s) + 1.5 O2 (g) → Fe2O3 (s) ∆H° = -824.2 kJ/mol.