Question 2.SP.11: Combining Heat Calculations Calculate the total heat, in jou......

Combining Heat Calculations
Calculate the total heat, in joules, needed to convert 15.0 g of liquid ethanol at 25.0 °C to gas at its boiling point of 78.0 °C. Ethanol has a specific heat of 2.46 J/g °C, and a heat of vaporization of 841 J/g.

Step-by-Step
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Step 1 List the grams of substance and change of state.
Given 15.0 g of ethanol at 25.0 °C; boiling point of ethanol 78.0  °C
Specific heat 2.46 J/g °C;  heat of vaporization 841 J/g

Need heat (J) to warm ethanol and change to gas at the boiling point

Step 2 Write the plan to convert grams to heat and desired unit. When several changes occur, draw a diagram of heating and changes of state.

Total heat = joules needed to warm ethanol from 25.0 °C to 78.0 °C (boiling point) + joules to change liquid to gas at 78.0 °C (boiling point)

Step 3 Write the heat conversion factors needed

\begin{matrix} SH_{\text{Ethanol}}=\frac{2.46  J}{g  °C} && 1  g  \text{of ethanol} (l \rightarrow g) = 841  J \\ \\ \frac{2.46  J}{g  °C}   and   \frac{g  °C}{2.46  J} && \frac{841  J}{\text{1 g ethanol}}  \text{and}   \frac{\text{1 g ethanol}}{841  J} \end{matrix}

Step 4 Set up problem with factors

ΔT = 78.0 °C – 25.0 °C = 53.0 °C

Heat needed to warm ethanol (liquid) at to ethanol (liquid) at 78.0 °C (boiling point):

15.0  \cancel {g}\times 53.0  \cancel {°C}\times \frac{2.46   J}{\cancel {g}  \cancel {°C}} =1960   J

Heat needed to change ethanol (liquid) to ethanol (gas) at 78.0 °C (boiling
point):

15.0  \cancel {\text{g ethanol}}\times \frac{841  J}{1  \cancel {\text{g ethanol}}}=12  600  J

Calculate the total heat:

\begin{matrix}\text{Heating ethanol}  (25.0 °C  \text{ to boiling point}  78.0  °C) &1 960  J \\ \text{Changing liquid to gas at boiling point}  (78.0 °C)& \underline{12 600  J}\\ \text{Total heat needed}&14 600  J& (\text{rounded off})\end{matrix}
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