21. consider the following chemical reaction: n2+ o2 2 no if 10.0 g of n2 reacts with excess oxygen then how many grams of no can be formed? a) 10.7 g b) 21.4 g c) 32.9 g d) 42.8 g page 4 of 8

The correct answer is Option B.

Explanation:

To calculate the number of moles, we use the equation:

  ....(1)

Given mass of nitrogen gas = 10 g

Molar mass of nitrogen gas = 28 g/mol

Putting values in above equation, we get:

The given chemical reaction follows:

As, oxygen gas is present in excess. Thus, it is considered as an excess reagent and nitrogen is considered as a limiting reagent because it limits the formation of products.

By Stoichiometry of the reaction:

1 mole of nitrogen gas produces 2 moles of nitrogen oxide.

So, 0.357 moles of nitrogen gas will produce = of nitrogen oxide.

Now, calculating mass of nitrogen oxide by putting values in equation 1, we get:

Moles of nitrogen oxide = 0.714 mol

Molar mass of nitrogen oxide = 30 g/mol

Putting values in equation 1, we get:

Hence, the correct answer is Option B.

answer:

the answer is 6 valence electrons.

explanation:

valence is the # of electrons on the outer most shell of an atom.

oxygen has 6.

although, the valency of oxygen is 2, because it only needs to make 2 covalent bonds, or gain 2 electrons, to achieve the stable octet configuration of a noble gas.

that's it!

if you need further assistance, let me know: )

~ trueboss72