Chemistry, 02.03.2020 17:55, shawnr6989
Calculate the amount of heat required to convert 10.0 grams of ice at –20.°C to steam at 120.°C. (Sp. heat of H2O(s) = 2.09 J/g•°C, Sp. heat of H2O(l) = 4.18 J/g•°C, Sp heat of H2O(g) = 2.03 J/g•°C; heat of fus. of H2O(s) = 333 J/g, heat of vap. of H2O(l) = 2260 J/g).
Answers: 3
![\Delta H=[m\times c_{p,s}\times (T_{final}-T_{initial})]+m\times \Delta H_{fusion}+[m\times c_{p,l}\times (T_{final}-T_{initial})]+m\times \Delta H_{vap}+[m\times c_{p,g}\times (T_{final}-T_{initial})]](/tpl/images/0530/2584/4a4bb.png)
= heat required for the reaction
= specific heat of solid water or ice = 
= specific heat of liquid water = 
= specific heat of gaseous water = 
= enthalpy change for fusion = 
= enthalpy change for vaporization = 
![\Delta H=[10.0g\times 2.09J/g^oC\times (0-(-20))^oC]+10.0g\times 333J/g+[10.0g\times 4.18J/g^oC\times (100-0)^oC]+10.0g\times 2260J/g+[10.0g\times 2.03J/g^oC\times (120-100)^oC]](/tpl/images/0530/2584/295b1.png)
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Calculate the amount of heat required to convert 10.0 grams of ice at –20.°C to steam at 120.°C. (Sp...
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