How many grams of carbon dioxide, CO₂, are present in a 0.150 L flask recorded at 525 mmHg and 32 ºC?

• A. 1.77 g
• B. 0.93 g
• C. 0.66 g
• D. 0.18 g
• E. 0.052 g

Answer: (D)

Verified step by step guidance

1. First, convert the temperature from degrees Celsius to Kelvin by adding 273.15 to the Celsius temperature: T(K) = 32 + 273.15.
2. Next, convert the pressure from mmHg to atm using the conversion factor: 1 atm = 760 mmHg. So, P(atm) = 525 mmHg / 760 mmHg/atm.
3. Use the Ideal Gas Law equation, PV = nRT, to solve for the number of moles (n) of CO2. Here, P is the pressure in atm, V is the volume in liters, R is the ideal gas constant (0.0821 L·atm/mol·K), and T is the temperature in Kelvin.
4. Rearrange the Ideal Gas Law equation to solve for n: n = PV / RT. Substitute the values for P, V, R, and T into the equation to find the number of moles of CO2.
5. Finally, convert the moles of CO2 to grams using the molar mass of CO2 (approximately 44.01 g/mol). Multiply the number of moles by the molar mass to find the mass in grams: mass (g) = n * 44.01 g/mol.