What is the volume in mL of 3.59 g CO2 of gas at 2.09 atm and -14 oC?

Given that:

                                           = 259.15 K

Now,

The number of moles of CO₂ will be:

=

=

=

By using the Ideal gas law, we get

→

or,

→    

By substituting the values, we get

or,

Thus the above answer is appropriate.

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800 ml is the volume in mL of 3.59 g CO2 of gas at 2.09 atm and -14°C.

Explanation:

Data given:

mass of the carbon dioxide gas = 3.59

pressure of the carbon dioxide gas =  2.09 atm

temperature of the carbon dioxide gas  = -14 degrees OR 273.15 +(-14) = 259.15 K

atomic mass of carbon dioxide =44.01 grams/mole

R = 0.0821 L.atm/mole K

volume occupied by the gas =?

number of moles of CO2 =

number of moles =

number of moles of carbon dioxide gas = 0.081 moles

from ideal gas law

PV = nRT

V =

V = 0.80 L is the volume of carbon dioxide gas

volume in ml = 0.8 x 1000

volume in ml= 800 ml

- lead + phosphoric acid = hydrogen + lead(ii) phosphate

i would say b

explanation:

but i think i would need more information than that