Question

When a $0.66g$sample of olive oil is burned in a calorimeter, the heat released increases the temperature of $370g$of water from $22.7^{\circ }\mathrm{C}$to $38.8^{\circ }\mathrm{C}$. What is the energy value for the olive oil in sample?

Short answer

The energy value of olive oil are$37.8KJ/g$in Kilojoule and$9.03Kcal/g$in Kilocalories.

Step-by-step solution

Given information

Calories include a certain total energy, indicated by calories burned. It promotes the execution of pharmacological biological functions.

Mass of olive oil$=0.66g$

Mass of Water$=370g$

Temperature varies from$22.7^{\circ }C$to$38.8^{\circ }C$

Find Energy in Kilojoule.

The rise in the temperature of $370g$ of water is${22.7}^{\circ }\mathrm{C}$to ${38.8}^{\circ }\mathrm{C}$when $0.66g$of olive oil is heated in calorimeter.

The amount of heat involved in the process in kilojoules is calculated as follows:

$Heat=specificheat\times mass\times ∆T$

On substitution of the respective values we have:

$Heat=specificheat\times mass\times ∆T$

$=4.184\frac{\mathrm{g}}{{\mathrm{g}}^{\circ }\mathrm{C}}\times 370\mathrm{g}\times \left({38.8}^{\circ }\mathrm{C}-22{.}^{\circ }\mathrm{C}\right)$

$=24,924J$

$=24.9KJ$

Thus, the heat added to burn the olive oil is $24.9KJ$, thus, the energy value of the olive oil is calculate as:

Energy value

$$\begin{gathered} =\frac{24.9KJ}{0.660g} \\ =37.9KJ/g \end{gathered}$$

The energy value of the olive oil is $37.8KJ/g$

Find Energy in Kilocalories.

The amount of heat consume in kcal is calculate as follows:

$Heatspecific=heat\times mass$

$=1.00\frac{\text{cal}}{{\mathrm{g}}^{\circ }\mathrm{C}}\times 370\mathrm{g}\times \left({38.8}^{\circ }\mathrm{C}-{22.7}^{\circ }\mathrm{C}\right)$

$=5,957cal$

$=5.9Kcal$

Thus, the heat added to burn the olive oil is $5.9Kcal$, thus, the energy value of the olive oil is calculated as :

Energy value

$$\begin{gathered} =\frac{5.9Kcal}{0.660g} \\ =9.03Kcal/g \end{gathered}$$

The energy value of the olive oil is $9.03Kcal/g$