Answer :
The volume is 30.9 mL that 38.8 g of CO2 occupies at 725 mmHg and 25.0°C.
To calculate the volume that 38.8 g of CO2 occupies at 725 mmHg and 25.0°C, we first need to use the ideal gas law equation, PV=nRT.
We can rearrange this equation to solve for volume: V=nRT/P.
We know the pressure is 725 mmHg and the temperature is 25.0°C, which is 298.15 K. We also need to determine the number of moles of CO2 present. To do this, we can use the molar mass of CO2, which is 44.01 g/mol.
38.8 g of CO2 is equal to 0.881 mol of CO2 (38.8 g / 44.01 g/mol).
Plugging in all of our values into the equation, we get: V = (0.881 mol x 0.08206 L·atm/mol·K x 298.15 K) / 725 mmHg.
Converting mmHg to atm, we get 0.954 atm.
Solving the equation, we get V = 0.0309 L, which is equivalent to 30.9 mL.
Therefore, 38.8 g of CO2 occupies a volume of 30.9 mL at 725 mmHg and 25.0°C.
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