given the following info for water molar heat of specific heat capacity of liquid water 4.18 j/g degrees calculate the total quanity of heat evolved when 10.0g of steam is condensed,cooled,and frozen to ice at -50 degrees
See your other post above.
To calculate the total quantity of heat evolved when steam is condensed, cooled, and frozen to ice, we need to consider the three steps involved:
1. Condensation of steam to liquid water.
2. Cooling of liquid water to its freezing point.
3. Freezing of liquid water to ice.
Step 1: Condensation of steam to liquid water
To calculate the heat evolved during condensation, we need to use the molar heat of vaporization of water. Unfortunately, that information is not provided in the question. Without the specific heat capacity of water vapor or the molar heat of vaporization, we cannot accurately calculate the heat evolved during condensation.
Step 2: Cooling of liquid water to freezing point
To calculate the heat evolved during cooling, we can use the specific heat capacity of liquid water, which is given as 4.18 J/g°C. However, the temperature to which the water needs to be cooled is not specified in the question. Without this information, we cannot proceed with the calculation.
Step 3: Freezing of liquid water to ice
To calculate the heat evolved during freezing, we need to use the molar heat of fusion of water, which is the heat required to freeze one mole of water (or convert one mole of water into ice) at the freezing point. Unfortunately, that information is not provided in the question.
Therefore, based on the information given in the question, we do not have enough data to calculate the total quantity of heat evolved when 10.0g of steam is condensed, cooled, and frozen to ice at -50 degrees.