How many grams of co2 gas would occupy 33.7 liters of volume at a temperature of -22.2 degrees Celsius and a pressure of 990 mm hg

The answer to your question is 93.88 grams

Explanation:

Data

mass of CO₂ = ?

Volume = 33.7 l

Temperature = -22.2°C

Pressure = 990 mmHg

constant of ideal gases = 0.082 atm l/mol°K

Process

1.- Convert temperature to °K

Temperature = -22.2 + 273

                      = 250.8°K

2.- Convert the pressure to atm

            1 atm 760 mmHg

            x       990 mmHG

                 x = (990 x 1) / 760

                 x = 1.3 atm

3.- Use the ideal gas law to find the moles of CO₂

           PV = nRT

-Solve for n

           n = PV/RT

-Substitution

           n = (1.3 x 33.7) / (0.082 x 250.8)

-Result

           n = 43.89 / 20.57

           n = 2.13

4.- Calculate the grams of CO₂

Molar mass CO₂ = 44g

                 44 g of CO₂ 1 mol

                   x                 2.13 moles

                   x = (2.13 x 44) / 1

                   x = 93.88 grams

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