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

Boy I'm really boutta get to yo pickle chin ahh boy, egg head like collard greens head a//ss boy, oh hell nah boy yo dirt ahh boy stank ahh boy afro head ahh, lip gloss chin ahh boy ugly ahh boi

Step-by-step explanation:

Answer 2

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

Step-by-step explanation:

To calculate the moles :

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

`\text{Moles of} CO=(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=
`(1)/(2)* 28=14moles` of
`O_2`

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

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