Question

how much oxygen is formed from 264g of co2 and 216g of h2o

Answer 1

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Answer : The amount of oxygen formed, 576 grams

Solution : Given,

Mass of CO_2 = 264 g

Mass of H_2O = 216 g

Molar mass of CO_2 = 44 g/mole

Molar mass of H_2O = 18 g/mole

First we have to calculate the moles of CO_2 and H_2O.

\text{Moles of }CO_2=\frac{\text{Mass of }CO_2}{\text{Molar mass of }CO_2}=\frac{264g}{44g/mole}=6moles

\text{Moles of }H_2O=\frac{\text{Mass of }H_2O}{\text{Molar mass of }H_2O}=\frac{216g}{18g/mole}=12moles

Now we have to calculate the limiting and excess reagent.

The balanced chemical reaction is,

6CO_2+6H_2O\rightarrow C_6H_{12}O_6+6O_2

From the balanced reaction we conclude that

As, 6 moles of CO_2 react with 6 moles of H_2O

So, 6 moles of CO_2 react with \frac{6}{6}\times 6=6 moles of H_2O

That means, in the given balanced reaction, CO_2 is a limiting reagent because it limits the formation of products and H_2O is an excess reagent.

The excess reagent remains (H_2O) = 12 - 6 = 6 moles

Now we have to calculate the moles of O_2.

As, 2 moles of CO_2 react with 6 moles of O_2

So, 6 moles of CO_2 react with \frac{6}{2}\times 6=18 moles of O_2

Now we have to calculate the mass of O_2.

\text{Mass of }O_2=\text{Moles of }O_2\times \text{Molar mass of }O_2

\text{Mass of }O_2=(18mole)\times (32g/mole)=576g

Therefore, the amount of oxygen formed, 576 grams

Answer 2

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