Answer:
2.87 g
Explanation:
Step 1: Given data
- Total pressure (P): 754.0 mmHg
- Partial pressure of water (pW): 17.55 mmHg
- Volume of gas (V): 1.62 L
Step 2: Calculate the partial pressure of CO₂
The total pressure is the sum of the partial pressures of CO₂and water.
P = pCO₂ + pW
pCO₂ = P - pW = 754.0 mmHg - 17.55 mmHg = 736.5 mmHg
We will convert this pressure to atm using the conversion factor 1 atm = 760 mmHg.
736.5 mmHg × 1 atm/760 mmHg = 0.9691 atm
Step 3: Calculate the moles (n) of CO₂
We will use the ideal gas equation.
P × V = n × R × T
n = P × V/R × T
n = 0.9691 atm × 1.62 L/(0.0821 atm.L/mol.K) × 293 K = 0.0653 mol
Step 4: Calculate the mass corresponding to 0.0653 moles of CO₂
The molar mass of CO₂ is 44.01 g/mol.
0.0653 mol × 44.01 g/mol = 2.87 g