ANSWER
EXPLANATION
Given that:
[tex]\begin{gathered} \text{ The mass of ice }=\text{ 6.83g} \\ \text{ initial temperature }=-12\degree C \\ \text{ Final temperature }=20\degree C \\ \text{ Specific heat capacity of ice }=\text{ 2.09 J/g}\degree C \\ \text{ }\Delta H_{Vapor}(H_2O)\text{ }=\text{ 40.7kJ/mol} \\ \text{ }\Delta H_{Fusion}(H_2O)\text{ }=\text{ 6.02 kJ/mol} \end{gathered}[/tex]
To find the heat required to convert ice to water, follow the steps below
Step 1: Write the heat formula
[tex]q\text{ }=\text{ mc}\Delta\theta[/tex]
Since, the ice will be converted to solid first, the the final final temperature will be 0 degrees Celcius
[tex]\begin{gathered} \text{ q }=\text{ 6.83}\times2.09\times\text{ \lbrack\lparen0-\lparen-12\rparen\rbrack} \\ \text{ q }=\text{ 6.83}\times2.09\times\text{ \lparen0 }+12) \\ \text{ q}=\text{ 6.83}\times\text{ 2.09}\times\text{ 12} \\ \text{ q }=\text{ 171.2964 J} \end{gathered}[/tex]
Step 2: find the heat required to convert the solid to liquid from 0 degrees Celcius to 0 degrees Celcius
[tex]\text{ q}=\text{ m }\times\text{ }\Delta H_{fus}[/tex]
Where m is the mass of the sample
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