Asample of he gas (3.0 l) at 5.6 atm and 25°c was combined with 4.5 l of ne gas at 3.6 atm and 25°c at constant temperature in a 9.0 l flask. the total pressure in the flask was atm. assume the initial pressure in the flask was 0.00 atm.

3.6667

Explanation:

For helium gas:

Using Boyle's law  

Given ,  

V₁ = 3.0 L

V₂ = 9.0 L

P₁ = 5.6 atm

P₂ = ?

Using above equation as:

The pressure exerted by the helium gas in 9.0 L flask is 1.8667 atm

For Neon gas:

Using Boyle's law  

Given ,  

V₁ = 4.5 L

V₂ = 9.0 L

P₁ = 3.6 atm

P₂ = ?

Using above equation as:

The pressure exerted by the neon gas in 9.0 L flask is 1.8 atm

Thus total pressure = 1.8667 + 1.8 atm = 3.6667 atm.

answer; economic order quantity;

since the atomic number is the number of protons in the nucleus, as we move to the left on the periodic table, the electrostatic pull between the nucleus and the valence electron shell decreases. as we move down a group (vertical column), the valence shell energy level gets further and further from the nucleus.