How many grams of carbon dioxide, CO₂, are present in a 0.150 L flask recorded at 525 mmHg and 32.0 ºC?

• A. 1.77 g
• B. 0.932 g
• C. 0.660 g
• D. 0.182 g
• E. 0.0521 g

Answer: (D)

Verified step by step guidance

1. Identify the known variables from the problem: volume (V) = 0.150 L, pressure (P) = 525 mmHg, temperature (T) = 32 ºC, and the gas is carbon dioxide (CO\_2).
2. Convert the pressure from mmHg to atmospheres (atm) because the ideal gas constant R is typically given in atm·L/(mol·K). Use the conversion: 1 atm = 760 mmHg, so \( P_{atm} = \frac{525}{760} \).
3. Convert the temperature from Celsius to Kelvin using the formula \( T(K) = T(ºC) + 273.15 \).
4. Use the Ideal Gas Law equation to find the number of moles (n) of CO\_2: \[ P V = n R T \] Rearranged to solve for n: \[ n = \frac{P V}{R T} \] where \( R = 0.0821 \) atm·L/(mol·K).
5. Calculate the mass of CO\_2 by multiplying the number of moles by the molar mass of CO\_2 (approximately 44.01 g/mol): \[ \text{mass} = n \times 44.01 \text{ g/mol} \].