How many grams of carbon monoxide are needed to react with an excess of iron (iii) oxide to produce 198.5 grams of iron? fe2o3(s) + 3co(g) à 3co2(g) + 2fe(s)

Answer : The grams of carbon monoxide needed are 148.89 g

Solution : Given,

Mass of iron, Fe = 198.5 g

Molar mass of iron, Fe = 56 g/mole

Molar mass of carbon monoxide, CO = 28 g/mole

First we have to calculate the moles of iron, Fe.

The balanced chemical reaction is,

From the balanced reaction, we conclude that

2 moles of iron produces from the 3 moles of carbon monoxide

3.545 moles of iron produces from the moles of carbon monoxide

Now we have to calculate the mass of carbon monoxide, CO.

Therefore, the grams of carbon monoxide needed are 148.89 g

Hello!

One way the modern atomic model differs from Thomson's atomic model is that electrons are no longer scattered throughout an atom's positive matter like chocolate chips in a cookie dough. instead, each electron is outside of the nucleus occupying a specific Energy Level.

The modern atomic model is also called the Schrodinger's model or the Quantum Mechanical model. Although atoms are commonly depicted like planets with electrons orbiting it like satellites, in reality, electrons aren't in fixed orbits but there are clouds where there is a bigger probability of finding an electron. This area is called an Energy Level. 

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