Answer:
0.56 atm
Explanation:
First of all, we need to find the number of moles of the gas.
We know that
m = 1.00 g is the mass of the gas
[tex]Mm=44.0 g/mol[/tex] is the molar mass of the carbon dioxide
So, the number of moles of the gas is
[tex]n=\frac{m}{M_m}=\frac{1.00 g}{44.0 g/mol}=0.023 mol[/tex]
Now we can find the pressure of the gas by using the ideal gas equation:
[tex]pV=nRT[/tex]
where
p is the pressure
[tex]V=1.00 L = 0.001 m^3[/tex] is the volume
n = 0.023 mol is the number of moles
[tex]R=8.314 J/mol K[/tex] is the gas constant
[tex]T=25.0^{\circ}+273=298 K[/tex] is the temperature of the gas
Solving the equation for p, we find
[tex]p=\frac{nRT}{V}=\frac{(0.023 mol)(8.314 J/mol K)(298 K)}{0.001 m^3}=5.7 \cdot 10^4 Pa[/tex]
And since we have
[tex]1 atm = 1.01\cdot 10^5 Pa[/tex]
the pressure in atmospheres is
[tex]p=\frac{5.7\cdot 10^4 Pa}{1.01\cdot 10^5 Pa/atm}=0.56 atm[/tex]
