Calculate the enthalpy change, Delta H, for the process in which 26.7 g of water
ID: 1048978 • Letter: C
Question
Calculate the enthalpy change, Delta H, for the process in which 26.7 g of water is converted from liquid at 7.3 degree C to vapor at 25.0 degree C For water, Delta H_vap = 44.0 kJ/mol at 25.0 degree C and C_s =4.18 J/(g middot degree C) forH_2O(l). Express your answer to three significant figures and include the appropriate units. How many grams of ice at -11.2 degree C can be completely converted to liquid at 19.1 degree C if the available heat for this process is 5.07 times 10^3 kJ? For ice, use a specific heat of 2.01 J/(g middot degree C) and Delta H_fus = 6.01kJ/mol. Express your answer to three significant figures and include the appropriate units.Explanation / Answer
Part B
q = m x C x DT
q = m x C x (Tf - Ti)
q = amount of heat energy gained or lost by substance
m = mass of sample
C = heat capacity (J oC-1 g-1 or J K-1 g-1)
Tf = final temperature
Ti = initial temperature
Using the same equation we can find out the weight of ice which undergoes following changes
The temperature of ice icreases to oC
Then it melts to ice to water
followed by water temperature goes up to 19.1 oC
Kilo joules are converted to joules
Let us keep weight of ice as Z
Z x 2.01 x (11.2) + Z x 6010 /18 + Z x 4.18 x 19.1 = 5070
22.512 Z + 333.88 Z + 79.84 Z = 5070
436.24 Z = 5070
Z = 11.622
The weight of ice equal to 11.622 gm
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