Answer :
Final answer:
To find the number of grams of O2 gas in the container, we can use the ideal gas law equation PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the ideal gas law constant, and T is the temperature.
Explanation:
To find the number of grams of O2 gas in the container, we can use the ideal gas law equation, which is PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the ideal gas law constant, and T is the temperature.
We are given the pressure (775 mmHg), volume (3700 mL), and temperature (33°C). To find the number of moles of O2, we need to rearrange the ideal gas law equation to solve for n.
n = PV / RT
Now, we can plug in the values and solve for n using the appropriate units. Once we have the number of moles, we can convert it to grams by multiplying it by the molar mass of O2.
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There are approximately **4.80 grams of oxygen gas** in the container.
Here's how to calculate the mass of oxygen gas in the container:
**1. Use the Ideal Gas Law:**
The Ideal Gas Law relates the pressure (P), volume (V), number of moles (n), and temperature (T) of a gas:
PV = nRT
where:
* R is the gas constant (0.0821 L atm/mol K)
**2. Rearrange the equation for n:**
We want to find the number of moles of oxygen gas (n_O2), so rearrange the equation:
n_O2 = PV / (RT)
**3. Plug in the known values:**
* P = 775 mmHg (convert to atm: 775 mmHg * 1 atm/760 mmHg ≈ 1.02 atm)
* V = 3700 mL (convert to L: 3700 mL * 1 L/1000 mL ≈ 3.70 L)
* T = 33°C + 273.15 K = 306.15 K
**4. Calculate the number of moles:**
n_O2 = (1.02 atm * 3.70 L) / (0.0821 L atm/mol K * 306.15 K) ≈ 0.150 mol
**5. Determine the mass of O2:**
Finally, use the molar mass of oxygen (32.00 g/mol) to find the mass:
mass_O2 = n_O2 * molar mass_O2
mass_O2 = 0.150 mol * 32.00 g/mol ≈ 4.80 g
Therefore, there are approximately **4.80 grams of oxygen gas** in the container.
