Question

Automobile catalytic converters use a platinum catalyst to reduce air pollution by changing emissions such as carbon monoxide, CO(g), into carbon dioxide, CO2(g). The uncatalyzed reaction is represented by the balanced equation below.2CO(g) O2(g) 2CO2(g) +heat. determine the mass of O2(g) required to completely react with 784g moles of CO(g) during this reaction.

Answer 1

Answer: 448 g of $O_2$ will be required to completely react with 784g moles of CO(g) during this reaction.

Explanation:

To calculate the moles :

$\text{Moles of solute}=\frac{\text{given mass}}{\text{Molar Mass}}$    

$\text{Moles of} CO=\frac{784g}{28g/mol}=28moles$

The balanced chemical equation is:

$2CO(g)+O_2(g)\rightarrow 2CO_2(g)$  

According to stoichiometry :

2 moles of $CO$ require  = 1 mole of $O_2$

Thus 28 moles of $CO$ will require=$\frac{1}{2}\times 28=14moles$  of $O_2$

Mass of $O_2=moles\times {\text {Molar mass}}=14moles\times 32g/mol=448g$

Thus 448g of $O_2$ will be required to completely react with 784g moles of CO(g) during this reaction.

Answer 2

Answer:

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Explanation: