Chemistry, 07.03.2020 05:14 spdesch2558
Calculate the amount of energy (in kilojoules) needed to heat 346 g of liquid water from –10 °C to 182°C. Assume that the specific heat of water is 4.184 J/g · °C for liquid and that the specific heat of steam is 1.99 J/g · °C.
Answers: 2
![\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/0537/8966/4a4bb.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=[346g\times 2.09J/g^oC\times (0-(-80))^oC]+346g\times 333J/g+[346g\times 4.184J/g^oC\times (100-0)^oC]+346g\times 2260J/g+[346g\times 1.99J/g^oC\times (180-100)^oC]](/tpl/images/0537/8966/7d24b.png)
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Calculate the amount of energy (in kilojoules) needed to heat 346 g of liquid water from –10 °C to 1...
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