How much energy is released to the environment by 50.0 grams of condensing water vapor? The heat of vaporization of water is 2260 J/g.
The correct answer and explanation is:
To calculate the energy released when 50.0 grams of water vapor condenses, you can use the formula: Q=m×LvQ = m \times L_v
Where:
- QQ is the heat energy released (in joules).
- mm is the mass of the water vapor (in grams).
- LvL_v is the heat of vaporization of water (in joules per gram).
From the problem, the values are:
- m=50.0 gm = 50.0 \, \text{g}
- Lv=2260 J/gL_v = 2260 \, \text{J/g}
Substitute the values into the formula: Q=50.0 g×2260 J/g=113,000 JQ = 50.0 \, \text{g} \times 2260 \, \text{J/g} = 113,000 \, \text{J}
So, 113,000 joules of energy are released when 50.0 grams of water vapor condenses.
Explanation:
The process of condensation involves the phase change from water vapor (gas) to liquid water. During this change, the water vapor releases energy to the surroundings. This energy is known as the latent heat of vaporization. The heat of vaporization is the amount of energy required to change 1 gram of a substance from liquid to gas without changing its temperature. In reverse, during condensation, this same amount of energy is released.
In this case, the heat of vaporization of water is given as 2260 J/g. Therefore, for each gram of water vapor that condenses, 2260 joules of energy are released. For 50.0 grams of water vapor, the total energy released can be calculated by multiplying the mass (50.0 grams) by the heat of vaporization (2260 J/g), resulting in 113,000 joules.
This released energy is typically transferred to the surrounding environment, and it plays an essential role in weather systems, such as in cloud formation and precipitation. The energy released during condensation helps in the cooling of the surrounding air.