Final answer:
To determine the grams of CO₂ produced from the limestone sample, the Ideal Gas Law is applied using the given pressure, volume, and temperature. The moles of CO₂ calculated are then converted to grams using its molecular weight.
Step-by-step explanation:
The problem requires using the Ideal Gas Law to find out how many grams of CO₂ were produced from the heated sample of dolomitic limestone. First, we need to convert the volume of CO₂ to standard temperature and pressure (STP) conditions using the equation PV=nRT, where:
- P = pressure in atm (convert 750 mmHg to atm by dividing by 760)
- V = volume in liters (75.0 mL converted to liters by dividing by 1000)
- n = moles of CO₂ (unknown)
- R = ideal gas constant (0.0821 L·atm/K·mol)
- T = temperature in kelvins (convert 20°C to K by adding 273.15)
Once we have calculated the moles of CO₂, we can convert to grams using the molecular weight of CO₂ (44.01 g/mol). The calculated mass of CO₂ is the answer we seek to find.