At 1 atm, how much energy is required to heat 57.0 g of H₂O(s) at -12.0°C to H₂O(g) at 175.0°C? STRATEGY: 1. Calculate the energy for each temperature change or phase change individually. a. The energy needed to heat 57.0 g of H₂O(s) from-12.0°C to its melting point. b. The energy needed to melt 57.0 g of H₂O(s) at its melting point. c. The energy needed to heat 57.0 g of H₂O (1) from the melting point to the boiling point. d. The energy needed to boil 57.0 g of H₂O(1) at its boiling point. e. The energy needed to heat 57.0 g of H₂O(g) from the boiling point to 175.0°C. 2. Sum the energies from each step and convert to kilojoules. Step 1. Heat, m-AT-SHI (57.0 g) (2.087.) (12.0°C) -1 - 1430 J Heath -m. AH fusion (57.0 g) (333.6 J/g) - 1.90 × 10¹ J Heat,¸ = m · AT - SH = (57.0 g) (4.184 g) (100 °C) = 23800 J Heatam. AH vaporization (57.0 g) (2257 J/g) = 1.29 × 10³ J -m-AT-SH(57.0 g) 57.0 g) (2.000) (75.0°C) = 8550 J Heat, m. Step 2. "What is the sum of the individual energies? total energy: Convert the sum from joules to kilojoules. total energy:
At 1 atm, how much energy is required to heat 57.0 g of H₂O(s) at -12.0°C to H₂O(g) at 175.0°C? STRATEGY: 1. Calculate the energy for each temperature change or phase change individually. a. The energy needed to heat 57.0 g of H₂O(s) from-12.0°C to its melting point. b. The energy needed to melt 57.0 g of H₂O(s) at its melting point. c. The energy needed to heat 57.0 g of H₂O (1) from the melting point to the boiling point. d. The energy needed to boil 57.0 g of H₂O(1) at its boiling point. e. The energy needed to heat 57.0 g of H₂O(g) from the boiling point to 175.0°C. 2. Sum the energies from each step and convert to kilojoules. Step 1. Heat, m-AT-SHI (57.0 g) (2.087.) (12.0°C) -1 - 1430 J Heath -m. AH fusion (57.0 g) (333.6 J/g) - 1.90 × 10¹ J Heat,¸ = m · AT - SH = (57.0 g) (4.184 g) (100 °C) = 23800 J Heatam. AH vaporization (57.0 g) (2257 J/g) = 1.29 × 10³ J -m-AT-SH(57.0 g) 57.0 g) (2.000) (75.0°C) = 8550 J Heat, m. Step 2. "What is the sum of the individual energies? total energy: Convert the sum from joules to kilojoules. total energy:
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Question
At 1 atm, how much energy is required to heat 57.0 g57.0 g of H2O(s)H2O(s) at −12.0∘C−12.0∘C to H2O(g)H2O(g) at 175.0∘C?
Transcribed Image Text:At 1 atm, how much energy is required to heat 57.0 g of H₂O(s) at -12.0°C to H₂O(g) at 175.0°C?
STRATEGY:
1. Calculate the energy for each temperature change or phase change individually.
a. The energy needed to heat 57.0 g of H₂O(s) from-12.0°C to its melting point.
b. The energy needed to melt 57.0 g of H₂O(s) at its melting point.
c. The energy needed to heat 57.0 g of H₂O (1) from the melting point to the boiling point.
d. The energy needed to boil 57.0 g of H₂O(1) at its boiling point.
e. The energy needed to heat 57.0 g of H₂O(g) from the boiling point to 175.0°C.
2. Sum the energies from each step and convert to kilojoules.
Step 1.
m · AT - SHI = (57.0 g) (2.087.) (120°C) =
Heath -m. AH fusion (57.0 g) (333.6 J/g) - 1.90 × 10¹ J
Heat - m
Heat
Heat ➡m. AH vaporization (57.0 g) (2257 J/g) 1.29 × 10³ J
Heate - m· AT · SHI = (57.0 g) (2.000) (75.0 °C) = 8550 J
Step 2.
What is the sum of the individual energies?
total energy:
- m. AT - SII = (57.0 g) (4.184) (100 °C) = 2
°C) = 23800 J
J
Convert the sum from joules to kilojoules.
total energy:
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