A rigid tank contains 0.66 mol of oxygen (O2). Find the mass of oxygen that must be withdrawn from the tank to lower the pressure of the gas from 43 atm to 17 atm. Assume that the volume of the tank and the temperature of the oxygen are constant during this operation. Answer in units of g.

12.8 g of must be withdrawn from tank

Explanation:

Let's assume gas inside tank behaves ideally.

According to ideal gas equation-

where P is pressure of , V is volume of , n is number of moles of , R is gas constant and T is temperature in kelvin scale.

We can also write,

Here V, T and R are constants.

So, ratio will also be constant before and after removal of from tank

Hence,

Here, and

So,

So, moles of must be withdrawn = (0.66 - 0.26) mol = 0.40 mol

Molar mass of = 32 g/mol

So, mass of must be withdrawn =

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.