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krystalhurst97
13.10.2019 •
Chemistry
How much heat in kilojoules is evolved in converting 2.00 mol of steam at 150 ∘c to ice at -55.0 ∘c? the heat capacity of steam is 1.84 j/g∘c and that of ice is 2.09 j/g∘c.
remember that if heat is leaving the system, then q is a negative number and if heat is entering the system, then q is a positive number.
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Ответ:
= 115.898 kJ
Explanation:
Heat evolved in converting 2.00 mol of steam at 150 ∘C to ice at -55.0 ∘C
Will be calculated in steps
Step 1; Heat evolved by steam from 150°C to 100°C
Heat = (2×18) g × 1.84 J/g°C × (150 -100)
= 3312 Joules
Step 2; Heat required to convert steam to water without change in temperature;
Heat = moles × Molar Latent heat of vaporization.
= 2 moles × 4.07 ✕ 104 J/mol
= 8.14 × 10^4 Joules
Step 3: Heat evolved by water from 100°C to 0°C.
Heat = mass × specific heat capacity × ΔT
= (2 × 18) × 4.18 J/g°C × 100
= 15,048 Joules
Step 4; Heat evolved in converting water at 0°C to ice at 0°
Heat = number of moles × molar latent heat of fusion
= 2 moles × 6000 j/mole
= 12 000 Joules
Step 5, heat evolved in converting ice at 0°C to -55°C
Heat = mass × specific heat capacity × ΔT
= (2×18) × 2.09 j/g°C × 55
= 4138.2 Joules
Total amount of heat evolved;
= 3312 J + 8.14 × 10^4 J + 15,048 J + 12 000 J + 4138.2 J
= 115,898.2 joules
= 115.898 kJ
Ответ: