The production of nox gases is an unwanted side reaction of the main engine combustion process that turns octane, c8h18, into co2 and water. if 85% of the oxygen in an engine is used to combust octane, and the remainder used to produce nitrogen dioxide, calculate how many grams of nitrogen dioxide would be produced during the combustion of 800 grams of octane.

Explanation:

Hello,

At first, the combustion of octane is illustrated as shown below:

Now, since 800 grams of octane are burned, we compute the moles of oxygen that reacted via stoichiometry:

As that is the combusting oxygen, we now look for the total oxygen that was employed by:

Therefore the 15% used in the NO₂ turns out:

Finally, for the NO₂ production:

The produced grams of NO₂ are:

Best regards.

calculate how many grams of ammonia can be produced from 4.21 grams of

n2 + 3h2 = 2nh3

my answer:

25.0g n2 x (1 mol/ 28.0gn2) x (2 mol nh3/ 1 mol n2) x (17.0g nh3/ 1 molnh3) = 30.36g n2

25.0g h2 x (1 mol h2/ 2.00g h2) x (2 mol nh3/ 3 mol h2) x (17.0g nh3/ 1 mol nh3) = 141.67g h2

lr = n2

i have no clue hope you find the answer