Question

How many grams of NO2 are produced when you have 4.44 grams of NO in the following reaction? 2NO-> 2NO2

Answer 1

`6.81g` of `NO_2`

Explanation:

Well, we first need to write the balanced equation, that is

`2NO+O_2->2NO_2`

As you can see here, the mole ratio between `NO_2` and `NO` is `2:2=1`.

We now need to convert `4.44g` of `NO` into moles.

`NO` has a molar mass of `30g"/"mol`.

So, `4.44g` of `NO` will be `(4.44cancelg)/(30cancelg"/"mol)=0.148mol` of `NO`

Since the mole ratio of `NO` and `NO_2` is `1`, then `0.148mol` of `NO_2` will be produced.

`NO_2` has a molar mass of `46g"/"mol`.

So, `0.148mol` of `NO_2` will be

`0.148cancel(mol)*46g"/"cancel(mol)=6.808~~6.81g` of `NO_2`