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Answer :
Final answer:
The total pressure in the container with both CO and CO₂ gases at a given temperature and volume is 9.787 atmospheres, calculated using the Ideal Gas Law.
Explanation:
The total pressure in the container can be calculated using the Ideal Gas Law, which is PV = nRT where P is pressure, V is volume, n is number of moles of gas, R is the ideal gas constant, and T is the temperature in Kelvin.
First, we need to find the number of moles of CO and CO₂.
- The molar mass of CO is 28.01 g/mol, and the molar mass of CO₂ is 44.01 g/mol.
- For CO: n (CO) = 5.00 g / 28.01 g/mol = 0.1785 mol
- For CO₂: n (CO₂) = 5.00 g / 44.01 g/mol = 0.1136 mol
The total moles of gas in the container is the sum of moles of CO and CO₂: n (total) = 0.1785 mol + 0.1136 mol = 0.2921 mol
Using the Ideal Gas Law:
PV = nRT
- P = (nRT) / V
- P = (0.2921 mol * 0.08206 Lmol⁻¹K⁻¹ * 323.15 K) / 0.7500 L
- P = 9.787 atm
Therefore, the total pressure in the container is 9.787 atm.
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