How much heat (in ) is evolved in converting 1.00 of steam at 150.0 to ice at -55.0? The heat capacity of steam is 2.01 and of ice is 2.09 .

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In the atmosphere, the partial pressure of water is much lower than 1atm, therefore gaseous water can exist at temperatures much lower than 100 degrees C. It takes 169,500 joules of heat to change 5.00g of ice at-15c to liquid water at 10.0c

To determine the amount of heat evolved in converting steam at 150.0°C to ice at -55.0°C, we need to consider the following steps:

Step 1: Determine the heat required to cool the steam from 150.0°C to 0°C.
Step 2: Determine the heat required to condense the steam at 100.0°C to liquid water at 100.0°C.
Step 3: Determine the heat required to cool the liquid water from 100.0°C to 0°C.
Step 4: Determine the heat required to freeze the liquid water at 0°C to ice at 0°C.
Step 5: Determine the heat required to cool the ice from 0°C to -55.0°C.

Now, let's calculate each step:

Step 1:
The heat capacity of steam is 2.01 J/g°C. We need to calculate the heat required to cool 1.00 g of steam from 150.0°C to 0°C.
Q1 = mass × specific heat capacity × temperature change
= 1.00 g × 2.01 J/g°C × (0°C - 150.0°C)
= -301.50 J

Step 2:
The heat of condensation for steam at 100.0°C is 40.7 J/g. We need to calculate the heat required to condense 1.00 g of steam at 100.0°C to liquid water at 100.0°C.
Q2 = mass × heat of condensation
= 1.00 g × 40.7 J/g
= 40.7 J

Step 3:
The heat capacity of liquid water is 4.18 J/g°C. We need to calculate the heat required to cool 1.00 g of liquid water from 100.0°C to 0°C.
Q3 = mass × specific heat capacity × temperature change
= 1.00 g × 4.18 J/g°C × (0°C - 100.0°C)
= -418.00 J

Step 4:
The heat of fusion for water at 0°C is 334 J/g. We need to calculate the heat required to freeze 1.00 g of liquid water at 0°C to ice at 0°C.
Q4 = mass × heat of fusion
= 1.00 g × 334 J/g
= 334 J

Step 5:
The heat capacity of ice is 2.09 J/g°C. We need to calculate the heat required to cool 1.00 g of ice from 0°C to -55.0°C.
Q5 = mass × specific heat capacity × temperature change
= 1.00 g × 2.09 J/g°C × (-55.0°C - 0°C)
= -114.45 J

Now, to determine the total heat evolved, we add up all the individual heat values:
Total heat evolved = Q1 + Q2 + Q3 + Q4 + Q5
= -301.50 J + 40.7 J - 418.00 J + 334 J - 114.45 J
= -458.25 J

Therefore, the amount of heat evolved in converting 1.00 g of steam at 150.0°C to ice at -55.0°C is -458.25 J.