A250 ml flask contains 3.4 g of neon gas at 45°c. calculate the pressure of the neon gas inside the flask.

The answer to your question is P = 17.73 atm

Explanation:

V = 250 ml = 0.25 liters (L)

mass = 3.4 g

Temperature = 45°C = 45 + 273 = 318°K

Pressure = ?

R = 0.082 atm L / mol°K

Atomic mass Ne = 20.18 g

Process

1.- Calcule moles of Neon

                           20.18 g of Ne ------------------ 1 mol

                              3.4 g of Ne -------------------  x

                                            x = (3.4 x 1)/20.18

                                            x = 0.17 moles of Neon

2.- Find pressure

Ideal gases formula             PV = nRT

                                                  P = 17.73 atm                                                                          

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