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A mixture consisting of 4.8 g of oxygen and 15 g of nitrogen is prepared in a container such that the total pressure is 730 mmhg. The partial pressure of oxygen in the mixture is:
Accepted Answer
To calculate the partial pressure of oxygen, we can use Dalton's Law of Partial Pressures, which states that the total pressure of a mixture of gases is equal to the sum of the partial pressures of the individual gases. Here's how to solve it:
1. Calculate the mole fraction of oxygen:
- Moles of oxygen (O2) = 4.8 g / 32 g/mol = 0.15 mol
- Moles of nitrogen (N2) = 15 g / 28 g/mol = 0.54 mol
- Total moles = 0.15 mol + 0.54 mol = 0.69 mol
- Mole fraction of oxygen (X(O2)) = 0.15 mol / 0.69 mol = 0.217
2. Calculate the partial pressure of oxygen:
- Partial pressure of oxygen (P(O2)) = X(O2)
Total pressure
- P(O2) = 0.217
730 mmHg = 158.4 mmHg
Therefore, the partial pressure of oxygen in the mixture is approximately 158.4 mmHg.
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