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Dahasolnce [82]
3 years ago
8

Write the complete balanced equation for the reaction between iron (III) oxide (Fe2O3) and water (H2O). You do not need to make

the subscripts smaller; just write them out as regular numbers. For example: Fe2O3
Chemistry
2 answers:
igomit [66]3 years ago
7 0
Fe2O3 + H2O → Fe2O3·H2O
This is a hydration reaction where the iron oxide is dissolved into the water.
Phoenix [80]3 years ago
5 0

Explanation:

An equation will be balanced if the number of reactants equals the number of products.  

The given reaction is as follows.

      Fe_{2}O_{3} + H_{2}O \rightarrow Fe(OH)_{3}

Number of atoms on reactant side are as follows.

  • Fe = 2
  • O = 4
  • H = 2

Number of atoms on product side are as follows.

  • Fe = 1
  • O = 3
  • H = 3

Thus, to balance the given equation we need to multiply H_{2}O on reactant side by 3 and Fe(OH)_{3} by 2 on the product side.

Therefore, the balanced chemical equation will be as follows.

      Fe_{2}O_{3} + 3H_{2}O \rightarrow 2Fe(OH)_{3}

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<u>Answer:</u> The percentage yield of aspirin is 38.02 %.

<u>Explanation:</u>

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

\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}      .....(1)

  • <u>For salicylic acid:</u>

Given mass of salicylic acid (C_7H_6O_3) = 10.09 g

Molar mass of salicylic acid (C_7H_6O_3) = 138.12 g/mol

Putting values in equation 1, we get:

\text{Moles of salicylic acid}=\frac{10.09g}{138.12g/mol}=0.0730mol

The chemical equation for the formation of aspirin follows:

C_7H_6O_3+C_4H_6O_3\rightarrow C_9H_8O_4+CH_3COOH

As, acetic anhydride is present in excess. So, it is considered as an excess reagent.

Thus, salicylic acid is a limiting reagent because it limits the formation of products.

By Stoichiometry of the reaction:

1 mole of salicylic acid produces 1 mole of aspirin.

So, 0.0730 moles of salicylic acid will produce = \frac{1}{1}\times 0.0730=0.0730mol of aspirin

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

Molar mass of aspirin = 180.16 g/mol

Moles of aspirin = 0.073 moles

Putting values in equation 1, we get:

0.073mol=\frac{\text{Mass of aspirin}}{180.16g/mol}\\\\\text{Mass of aspirin}=13.15g

To calculate the percentage yield of aspirin, we use the equation:

\%\text{ yield}=\frac{\text{Experimental yield}}{\text{Theoretical yield}}\times 100

Experimental yield of aspirin = 5.0 g

Theoretical yield of aspirin = 13.15 g

Putting values in above equation, we get:

\%\text{ yield of aspirin}=\frac{5.0g}{13.15g}\times 100\\\\\% \text{yield of aspirin}=38.02\%

Hence, the percent yield of aspirin is 38.01 %.

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