Answer: The pressure of the gas is 4.4334atm.
Explanation:
The ideal gas law for pressure is shown as: [tex]P=\frac{nRT}{V}[/tex].
~n=number of moles (mol)
~R=ideal gas constant=[tex]0.0821\frac{L*atm}{mol*K}[/tex]
~T=temperature (K)
~V= volume (L)
We are not given the number of moles, but we can find that with the grams of CO₂ that we were given. This is also better because we have the compound as well, making it easier to find its molar mass on the periodic table.
[tex]8.06gCO_{2} *\frac{1molCO_{2} }{44.009gCO_{2} }=0.18molCO_{2}[/tex]
Now we are ready to plug our given information into the formula for the ideal gas law of pressure.
[tex]P=\frac{0.18mol*0.0821\frac{L*atm}{mol*K}*300K }{1.00L}[/tex] [tex]P=4.4334atm[/tex]
Given the work above, the pressure of the gas is 4.4334 atmospheres.
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