Calculate the mass of nitrogen dissolved at room temperature in an 86.0 l home aquarium. assume a total pressure of 1.0 atm and a mole fraction for nitrogen of 0.78.

Mass of nitrogen gas dissolved= 1.1732 grams

Explanation:

According to Dalton's Law of partial pressure:

Where,

is the partial pressure of nitrogen

is the Total pressure

is the mole fraction of nitrogen

Given :

Total pressure  = 1.0 atm

Mole fraction of nitrogen = 0.78

Partial pressure of nitrogen:

Partial pressure of nitrogen = 0.78 atm

According to Henry's law:

Solubility = Henry's constant (k)×Partial pressure

k = 6.26×10⁻⁴ mol/L-atm

Thus,

Solubility of nitrogen = 6.26×10⁻⁴ mol/L-atm×0.78 atm = 4.8828×10⁻⁴ mol/L

Given: Volume = 86.0 L

So, Moles of nitrogen gas dissolved:

Moles = Solubility (Concentration dissolved)×Volume

Moles = 4.8828×10⁻⁴ mol/L×86.0 L = 0.0419 moles

Also,

Molar mass of nitrogen gas = 28 g/mol

So,

Mass of nitrogen gas dissolved = 0.0419 moles×28 g/mol = 1.1732 grams

the number of valence electrons for each molecule or ion is shown beneath the structure. remember hydrogen will not have more than two electrons. this hydrogen is part of a covalent bond (sharing two electrons). a double bond here would cause hydrogen to share four electrons with phosphorus.

2b2t

explanation:

2b2t