To solve this problem, we can use the ideal gas law:
PV = nRT
Where:
P = pressure (in atmospheres)
V = volume (in liters)
n = number of moles
R = gas constant (0.0821 L.atm/(mol.K))
T = temperature (in Kelvin)
First, let's convert the given values:
Mass of CO2 (m) = 20g
Molar mass of CO2 (M) = 44.01 g/mol
Number of moles (n) = m/M = 20g / 44.01 g/mol = 0.454 mol
Volume (V) = 2250 mL = 2250/1000 L = 2.25 L
Pressure (P) = 5 atm
Now, let's solve for temperature (T):
PV = nRT
T = PV / nR
T = (5 atm) * (2.25 L) / (0.454 mol * 0.0821 L.atm/(mol.K))
T = 54.9 ℃
Therefore, the answer is E) 54.9 ℃.
what is the temperature in ℃ of 20g of CO2 in a 2250ml vessel if the pressure is 5 atmosphere? A31.5℃ B28.46℃ C2.98℃ D276℃ E54.9℃?
1 answer