What is the mass, in grams, of 0.125 L of CO2 at a temperature of 273 K and a pressure of 760 torrs?

0.25 g

Explanation:

We'll begin by writing the number of mole of CO₂. This can be obtained as follow:

Volume (V) = 0.125 L

Temperature (T) = 273 K

Pressure (P) = 760 torr = 1 atm

Gas constant (R) = 0.0821 atm.L/Kmol

Number of mole (n) =?

PV = nRT

1 × 0.125 = n × 0.0821 × 273

0.125 = n × 22.4133

Divide both side by 22.4133

n = 0.125 / 22.4133

n = 0.0056 mole

Finally, we shall determine the mass of 0.0056 mole of CO₂. This can be obtained as follow:

Number of mole of CO₂ = 0.0056 mole

Molar mass of CO₂ = 12 + (2×6)

= 12 + 32

= 44 g/mol

Mass of CO₂ =?

Mass = mole × molar mass

Mass of CO₂ = 0.0056 × 44

Mass of CO₂ = 0.25 g

Thus, the mass of CO₂ is 0.25 g

93.2 ml + 3920 ml = 4013 ml total  

(93.2 ml) * (2.03 m) / (4013 ml) = 0.0471 m

the volume in in l of the diluted solution would be 0.0471 m.

43.452

step-by-step explanation:

284 times .153 = 43.452