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The task asks for solving a problem involving a steel container holding oxygen under certain conditions, and it requires calculations in two parts:

1. **Part (a): Calculating the Mass of Oxygen in the Container**

   - **Given**:
     - Volume (\( V \)) = 25.0 liters = 0.025 m³ (1 liter = 0.001 m³)
     - Pressure (\( P \)) = 21.2 bar = 2,120,000 Pa (1 bar = 100,000 Pa)
     - Temperature (\( T \)) = 45°C = 318.15 K (45 + 273.15)
     - Gas constant (\( R \)) for oxygen = 8.314 J/(mol·K)

   - Use the ideal gas law to find the number of moles (\( n \)) of oxygen:
     \[
     PV = nRT \implies n = \frac{PV}{RT}
     \]
     Substituting values:
     \[
     n = \frac{2,120,000 \, \text{Pa} \times 0.025 \, \text{m}^3}{8.314 \, \text{J/(mol·K)} \times 318.15 \, \text{K}}
     \]

   - After finding \( n \), convert moles to mass using the molar mass of oxygen (\( M \)) which is approximately 32 g/mol:
     \[
     m = n \times M
     \]

2. **Part (b): Calculating the Temperature Rise Per Minute**

   - **Given**:
     - Power (\( P \)) = 250 W
     - Heat that actually goes into heating the oxygen = 90% of 250 W = 225 W
     - Time = 1 minute = 60 seconds

   - Use the formula for heat transfer:
     \[
     Q = P \times t
     \]
     where \( Q \) is the heat transferred, \( P \) is the power, and \( t \) is time.

   - To find the temperature rise (\( \Delta T \)), use the formula:
     \[
     Q = m \times c \times \Delta T \implies \Delta T = \frac{Q}{m \times c}
     \]
     - \( c \) is the specific heat capacity of oxygen, which is approximately \( 0.918 \, \text{J/g·K} \).

   - Substitute the values and calculate \( \Delta T \).

Let's solve these steps and provide the final answer.The solutions to the problem are as follows:

1. **Mass of Oxygen in the Container**: Approximately \( 641.19 \, \text{g} \).
2. **Temperature Rise Per Minute**: About \( 22.94 \, \degree \text{C/min} \).

It seems the provided solution in the problem statement mentions a temperature rise of \( 32 \, \degree \text{C/min} \). This difference could arise due to approximations or assumptions regarding specific heat or heat losses.

Would you like a more detailed explanation of the solution or any clarification on the steps? Here are a few related questions to deepen understanding:

1. How does the ideal gas law change if the gas is not ideal?
2. What would happen to the temperature rise if only 80% of the power was used for heating?
3. How does changing the volume of the container affect the mass of the gas inside?
4. What is the role of specific heat capacity in the heating process?
5. How would the calculations change if the gas was under a varying pressure?

**Tip**: Always double-check unit conversions, as they can significantly affect the final results in physics and chemistry problems!

There is a 25.0-liter steel container filled with oxygen at 21.2 bar and 45°C. Heat energy is added to the container at a rate of 250 W, of which 90% heats the oxygen. Calculate the mass of oxygen and the temperature rise per minute.

Learn how to calculate the mass of oxygen in a pressurized steel container and determine the temperature rise per minute using the ideal gas law and heat transfer formulas. The problem involves physics and chemistry concepts like the ideal gas law and heat transfer, suitable for students in Grades 10-12.

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