Asked Nov 20, 2019
3. What mass of Fe is required to react with 455 mL of oxygen at 22 °C and a
pressure of 725 torr according to the following equation?
4 Fe (s) +3 O2 (g) 2 Fe2O3 (s)

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3. What mass of Fe is required to react with 455 mL of oxygen at 22 °C and a pressure of 725 torr according to the following equation? 4 Fe (s) +3 O2 (g) 2 Fe2O3 (s) 46


Expert Answer

Step 1

The gaseous state is the state of matter with least intermolecular force of attraction between molecules and highest kinetic energy. The standard properties of gases like Pressure, volume, and temperature can be calculated with the help of ideal gas equation.

The ideal gas equation can be written as:


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P x V n x R x T Here P Pressure V volume T temperature R gas constant = 0.08314 L.atm/K.mol = moles of gas

Step 2

Pressure = 725 torr = 0.954 atm (1 atm = 760 torr)

Volume = 455 mL = 455 x 10-3 L

Temperature = 22C = 22 +273 = 295 K

Calculate number of moles of oxygen gas with the help of Ideal gas equation:


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P x V n x Rx T 0.954 atm x 455x 103 L nx 0.08314 L.atm/K.mol x 295 K 0.954 atm x 455x 103 L 0.08314 L.atm/K.mol x 295 K 17.7 x103 moles n

Step 3

According to balance chemical equation:

4 mole...


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4 moles Fe 17.7 x103 moles O2 -=23.6x103 moles Fe 3 moles O


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