The density of liquid oxygen at its boiling point is 1.14 kg/L, and its heat of vaporization is 213 kJ/kg .
How much energy in joules would be absorbed by 3.0 L of liquid oxygen as it vaporized?
Express your answer to two significant figures and include the appropriate units.

To find the energy absorbed by 3.0 liters of liquid oxygen during vaporization, we can use the given information and the following steps:

1. **Convert the volume to mass**: We are given the density of liquid oxygen as 1.14 kg/L. The mass of oxygen can be calculated using the formula:
   
   \[
   \text{mass} = \text{density} \times \text{volume}
   \]

   \[
   \text{mass} = 1.14 \, \text{kg/L} \times 3.0 \, \text{L} = 3.42 \, \text{kg}
   \]

2. **Calculate the energy**: The heat of vaporization of oxygen is given as 213 kJ/kg. The energy required to vaporize the liquid oxygen is:

   \[
   \text{energy} = \text{mass} \times \text{heat of vaporization}
   \]

   \[
   \text{energy} = 3.42 \, \text{kg} \times 213 \, \text{kJ/kg} = 728.46 \, \text{kJ}
   \]

3. **Convert kJ to J**: Since 1 kJ = 1000 J, we convert the result into joules:

   \[
   \text{energy} = 728.46 \, \text{kJ} \times 1000 = 728460 \, \text{J}
   \]

4. **Round to two significant figures**:

   \[
   \text{energy} \approx 7.3 \times 10^5 \, \text{J}
   \]

Thus, the energy absorbed by 3.0 L of liquid oxygen as it vaporizes is approximately **7.3 × 10⁵ J**.

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Would you like more details or have any questions on this?

Here are five related questions:
1. How would the energy change if the volume of liquid oxygen was doubled?
2. What is the relationship between density and volume when calculating mass?
3. How does the heat of vaporization vary for different substances?
4. What happens to the energy during the vaporization process at the molecular level?
5. How can you convert between joules and kilocalories?

**Tip**: Always check the units and convert them appropriately to avoid calculation errors.

The density of liquid oxygen at its boiling point is 1.14 kg/L, and its heat of vaporization is 213 kJ/kg. How much energy in joules would be absorbed by 3.0 L of liquid oxygen as it vaporized? Express your answer to two significant figures and include the appropriate units.

Learn how to calculate the energy absorbed by 3.0 L of liquid oxygen during vaporization. This problem explores key concepts like density, mass calculation, and unit conversion, using the heat of vaporization (213 kJ/kg) and a density of 1.14 kg/L. The final answer is expressed in joules to two significant figures.

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