What is the mass, in grams, of 0.125 L of CO2 at a temperature of 273 K and a pressure of 760 torrs? July 22, 2021 by Verity What is the mass, in grams, of 0.125 L of CO2 at a temperature of 273 K and a pressure of 760 torrs?
Answer: 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 Reply
Answer:
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