For questions , refer to the following table.
$\begin{array}{lc}
\hline \text { Substance } & \text { Specific Heat Capacity }\left(\mathrm{J} / \mathrm{g}{ }^{\circ} \mathrm{C}\right) \
\hline \text { Gold }(\mathrm{Au}) & 0.129 \
\text { Copper (Cu) } & 0.386 \
\text { Iron (Fe) } & 0.450 \
\text { Aluminum (Al) } & 0.900 \
\text { Ethanol }\left(\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}\right) & 2.460 \
\hline
\end{array}$
-A 176 g sample of ethanol was provided 30 kJ of heat energy. Afterwards, the temperature of the sample was found to be 75 °C. What was the initial temperature of the sample?

Question

For questions , refer to the following table.
 $\begin{array}{lc}
\hline \text { Substance } & \text { Specific Heat Capacity }\left(\mathrm{J} / \mathrm{g}{ }^{\circ} \mathrm{C}\right) \
\hline \text { Gold }(\mathrm{Au}) & 0.129 \
\text { Copper (Cu) } & 0.386 \
\text { Iron (Fe) } & 0.450 \
\text { Aluminum (Al) } & 0.900 \
\text { Ethanol }\left(\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}\right) & 2.460 \
\hline
\end{array}$
-A 176 g sample of ethanol was provided 30 kJ of heat energy. Afterwards, the temperature of the sample was found to be 75 °C. What was the initial temperature of the sample?

Quizplus · Accepted Answer

The initial temperature can be calculated using the formula $ q = mc\Delta T $. Rearranging gives $\Delta T = \frac{q}{mc}$. Substituting the given values: $ q = 30000 \, \text{J} $, $ m = 176 \, \text{g} $, $ c = 2.460 \, \text{J/g°C} $, we find $\Delta T = \frac{30000}{176 \times 2.460} \approx 69 \, \text{°C} $. Since the final temperature is 75 °C, the initial temperature is $ 75 - 69 = 6 \, \text{°C} $.

For Questions , Refer to the Following Table -A 176 G Sample of Ethanol Was Provided 30 KJ