An important reaction that takes place in a blast furnace during the production of iron is the formation of iron metal and CO2 from Fe2O3 and CO. Part A Find the mass of Fe2O3 required to form 930 kg of iron. Express your answer with the appropriate units.

The mass of Fe2O3 required is 1328.56 Kg.

The equation of the reaction is;

Fe2O3 + 3CO > 2Fe +  3CO2

From the question, we are told that the mass of iron formed is 930 kg.

Number of moles in 930 kg of iron = 930 × 10^3 g/56 g/mol

= 16607 moles of iron

Based on the stoichiometry of the reaction;

1 mole of Fe2O3 is required to produce 2 moles of iron

x moles of Fe2O3 is required to produce 16607 moles of iron

x = 1 mole × 16607 moles /2 moles

x = 8303.5 moles

Mass of Fe2O3 =  8303.5 moles × 160 g/mol

Mass of Fe2O3 = 1328.56 Kg

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Mass of required to form 930 kg of iron is 1328 kg

Explanation:

To calculate the number of moles, we use the equation:

     .....(1)

For iron:

Given mass of iron = 930 kg = 930000 g  (1kg=1000g)

Molar mass of iron = 56 g/mol

Putting values in equation 1, we get:

The chemical equation for the  production of iron  follows:

By Stoichiometry of the reaction:

2 moles of iron are  produced by =  1 mole of

So, 16607 moles of iron will be produced by = of

Now, calculating the mass of from equation 1, we get:

Mass of =

Thus mass of required to form 930 kg of iron is 1328 kg

in 1783 cavendish was working with his hydrogen gas and found that when he burned it and condensed the vapor it was water. this was very significant since it disproved the greek theory of elements completely since water was not a simple substance but the product of two gases. it was lavoisier who hearing of the experiment gave cavendish's gas the name hydrogen ("water-producer") and added that hydrogen burned by combining with oxygen and that water was a hydrogen-oxygen combination.

explanation:

i would say b

explanation:

but i think i would need more information than that