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Q = ms  T

Calculate the total quantity of heat evolved when 10.0g of steam at 200  C is condensed, cooled , and frozen to ice at -50  C. The specific heat capacity of ice and steam are 2.06J/g  C and 2.03J/g  C respectively. 1. 2. 3. 4. 5. 1. Q = ms  T. Q = (10.0g)(2.03J/g  C)(100  C).

rachel-puckett
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Q = ms  T

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  1. Calculate the total quantity of heat evolved when 10.0g of steam at 200 C is condensed, cooled , and frozen to ice at -50 C. The specific heat capacity of ice and steam are 2.06J/gC and 2.03J/gC respectively. 1 2 3 4 5

  2. . 1 Q = msT Q = (10.0g)(2.03J/gC)(100C) Q = 2030J = 2.030kJ 1

  3. 2 n(H2O) = mass / molar mass = 10.0g / 18g mol-1 = 0.56 mol H2O vap H (H2O) = 40.6kJ/mol vap H (H2O) = 0.56 mol  40.6 kJ/mol = 22.7 kJ 2

  4. 3 Q = msT Q = (10.0g)(4.18J/gC)(100C) Q = 4180J = 4.180kJ 3

  5. 4 n(H2O) = mass / molar mass = 10.0g / 18g mol-1 = 0.56 mol H2O fus H (H2O) = 40.6kJ/mol fus H (H2O) = 0.56 mol  40.6 kJ/mol = 22.74 kJ 4

  6. 5 Q = msT Q = (10.0g)(2.06J/gC)(50C) Q = 1030J = 1.030kJ 5

  7. Calculate the total quantity of heat evolved when 10.0g of steam at 200 C is condensed, cooled , and frozen to ice at -50 C. Total heat = 2.030kJ + 22.7 kJ + 4.180kJ + 22.74 kJ + 1.030kJ = 52.68kJ

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