Question

Nitrogen monoxide is produced by combustion in an automobile engine. For the following reaction, 4.36 grams of nitrogen monoxide are mixed with excess oxygen gas . The reaction yields 5.46 grams of nitrogen dioxide . nitrogen monoxide ( g ) oxygen ( g ) nitrogen dioxide ( g ) What is the theoretical yield of nitrogen dioxide

Answer 1

`6.68~g~NO_2`

Step-by-step explanation:

We have to start with the combustion reaction:

`NO~+~O_2~->~NO_2`

Then we can balance the reaction:

`2NO~+~O_2~->~2NO_2`

If we want to find the theoretical yield, we have to calculate the amount of
`NO_2`. To do this, we have to first convert the 4.36 g of
`NO` to moles
`NO` (using the molar mass 30 g/mol), then we have to convert from moles of
`NO` to moles of
`NO_2` (using the molar ratio) finally, we have to convert from moles of
`NO_2` to grams of
`NO_2` (using the molas mass 46 g/mol), so:

`4.36~g~NO(1~mol~NO)/(4.36~g~NO)(2~mol~NO_2)/(2~mol~NO)(46~g~NO_2)/(1~mol~NO_2)=6.68~g~NO_2`

I hope it helps!