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4 years ago

The decomposition of 11.0 g of fe2o3 results in

1 answer:

7 0

2Fe2O3=4Fe+3O2
1 mole Fe2O3=56*2+3*16=160g
2*160g Fe2O3.....4*56gFe.....6*16g O
11gFe2O3....x g Fe....y g O
x=11*4*56/(2*160)=7.7 g Fe
y=11*6*16/(2*160)=3.3g O

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3 years ago

How many grams of na2co3 would be needed to produce 1000g of nahco3

Ivenika [448]

Answer:

630.95 grams of Na₂CO₃ would be needed to produce 1000g of NaHCO₃

Explanation:

The balanced reaction is:

Na₂CO₃ + CO₂+ H₂O → 2 NaHCO₃

By stoichiometry of the reaction (that is, the relationship between the amount of reagents and products in a chemical reaction), the following amounts of each compound participate in the reaction:

Na₂CO₃: 1 moles
CO₂: 1 mole
H₂O: 1 mole
NaHCO₃: 2 moles

Being the molar mass:

Na₂CO₃: 106 g/mole
CO₂: 44 g/mole
H₂O: 18 g/mole
NaHCO₃: 84 g/mole

Then by stoichiometry the following quantities of mass participate in the reaction:

Na₂CO₃: 1 mole* 106 g/mole= 106 g
CO₂: 1 mole* 44 g/mole= 44 g
H₂O: 1 mole* 18 g/mole= 18 g
NaHCO₃: 2 moles* 84 g/mole= 168 g

You can apply the following rule of three: if 106 grams of Na₂CO₃ are needed to produce 168 grams of NaHCO₃, how much mass of Na₂CO₃ is necessary to produce 1000 grams of NaHCO₃?

$mass of Na_{2} CO_{3}=\frac{1000grams ofNaHCO_{3} *106gramsofNa_{2} CO_{3} }{168grams ofNaHCO_{3}}$

mass of Na₂CO₃= 630.95 grams

630.95 grams of Na₂CO₃ would be needed to produce 1000g of NaHCO₃

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3 years ago