Answer:
Pressure = 0.592 atm
Explanation:
To find the pressure of the CO2 gas in the cylinder, you can use the Ideal Gas Law:
=
PV=nRT
where:
P = pressure (in atm)
V = volume (in liters)
n = number of moles of gas
R = ideal gas constant (0.0821 L·atm/(K·mol))
T = temperature (in Kelvin)
Steps to solve:
Calculate the number of moles (
n) of CO2:
First, find the molar mass of CO2. The atomic masses are:
Carbon (C) = 12.01 g/mol
Oxygen (O) = 16.00 g/mol
Molar mass of CO2 = 12.01 + 2 × 16.00 = 44.01 g/mol
Number of moles (
n) is calculated by:
=
mass
molar mass
n=
molar mass
mass
=
18.7
g
44.01
g/mol
n=
44.01 g/mol
18.7 g
≈
0.425
mol
n≈0.425 mol
Use the Ideal Gas Law to find the pressure:
Rearrange the Ideal Gas Law to solve for
P:
=
P=
V
nRT
Plug in the values:
=
0.425
mol
n=0.425 mol
=
0.0821
L
\cdotp
atm/(K
\cdotp
mol)
R=0.0821 L\cdotpatm/(K\cdotpmol)
=
455
K
T=455 K
=
26.5
L
V=26.5 L
=
0.425
×
0.0821
×
455
26.5
P=
26.5
0.425×0.0821×455
≈
15.690
26.5
P≈
26.5
15.690
≈
0.592
atm
P≈0.592 atm
