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yellowmanatee878Lv1

19 May 2020

In an experiment, of powdered iron (III) oxide is mixed with carbon and heated to in a rigid reactor.

The following reaction occurred:

Assume that the reaction is complete, the volume of Fe(s) and C(s) is small enough to be ignored, and the temperature of the reactor is maintained at .

1. Write the balanced reaction.

2. Calculate the number of moles of gas formed.

3. What will be the pressure of the gas in the reactor after the reaction?

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burgundysheep393Lv1

2 Jun 2021

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Related questions

In an experiment, of powdered iron (III) oxide is mixed with carbon and heated to in a rigid reactor.

The following reaction occurred:

Assume that the reaction is complete, the volume of and is small enough to be ignored, and the temperature of the reactor is maintained at .

1. Write the balanced reaction.

2. Calculate the number of moles of gas formed.

3. What will be the pressure of the gas in the reactor after the reaction?

graybeaver739

Q1) chemist has to titrate an acid with a molecular formula containing only carbon, hydrogen, and oxygen with the respective percentages: 53.66% (C), 4.09% (H) and 42.25% (O) by mass. To reach the equivalence point the chemist used 18.02 mL of NaOH solution 0.0406 (M) to neutralize 0.3602 g of this acid. Assuming that the acid is monoprotic (there is only one acidic hydrogen per molecule of acid): 1. Calculate the number of mole of acid used in the titration. 2. What is the empirical formula of the acid? 3. What is the molecular formula of the acid?

Q2) In an experiment 26.0 g of powdered iron (III) oxide is mixed with 3g carbon and heated to 500°C in a rigid 6.0 L reactor. The following reaction occurred:

Assume that the reaction is 100% complete, the volume of Fe(s) and C(s) is small enough to be ignored, and the temperature of the reactor is maintained at 500 °C.