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What type of reaction is this? A Synthesis reaction, decomposition, or replacement?

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RUDIKE [14]4 years ago

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The process involved in this problem are :

$(1):H_2O(s)(0^oC)\rightarrow H_2O(l)(0^oC)\\\\(2):H_2O(l)(0^oC)\rightarrow H_2O(l)(32.0^oC)$

The expression used will be:

$\Delta H=m\times \Delta H_{fusion}+[m\times c_{p,l}\times (T_{final}-T_{initial})]$

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$c_{p,l}$ = specific heat of liquid water = $1cal/g^oC$

$\Delta H_{fusion}$ = enthalpy change for fusion = $80.0cal/g$

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$\Delta H=17g\times 80.0cal/g+[17g\times 1cal/g^oC\times (32.0-0)^oC]$

$\Delta H=1904cal$

Therefore, the heat required is, 1904 calories.

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