You are provided with 2.80 mol of nitrogen monoxide gas. using the balanced chemical equation completed in part a, determine how many moles of oxygen gas are needed to completely react with the nitrogen monoxide gas, and how many moles of nitrogen dioxide are formed as a result?

1.40 moles of O₂, and 2.80 moles of NO₂

Explanation:

The balanced reaction of nitrogen monoxide (NO) with oxygen (O₂) is:

2NO(g) + O₂(g) → 2NO₂(g)

We can notice that the stoichiometry is 2 moles of NO: 1 mole of O₂: 2 moles of NO₂, thus, for 2.80 mol of NO:

2 moles of NO 1 mol of O₂

2.80 moles       x

By a simple direct three rule:

2x = 2.80

x = 1.40 moles of O₂

2 moles of NO 2 moles of NO₂

2.80 moles       y

By a simple direct three rule:

y = 2.80 moles of NO₂.

the answer is option a.

the seeing the electronic configuration we can say that the element is fluorine.

fluorine is the most electronegative element in the periodic table.

but by only seeing the configuration we cannot say about its reactivity because we don't know if its configuration after excitation or by addition of electrons.

but if not then, it is the lightest halogen and exists as a highly toxic pale yellow diatomic gas at standard conditions. as the most electronegative element, it is extremely reactive: almost all other elements, including some noble gases, form compounds with fluorine.