Answer:
C. 7370 joules.
Explanation:
There is a mistake in the statement. Correct form is described below:
<em>Using the above data table and graph, calculate the total energy in Joules required to raise the temperature of 15 grams of ice at -5.00 °C to water at 35 °C. </em>
The total energy needed to raise the temperature is the combination of latent and sensible heats, all measured in joules, and represented by the following model:
![Q = m\cdot [c_{i} \cdot (T_{2}-T_{1})+L_{f} + c_{w}\cdot (T_{3}-T_{2})]](https://tex.z-dn.net/?f=Q%20%3D%20m%5Ccdot%20%5Bc_%7Bi%7D%20%5Ccdot%20%28T_%7B2%7D-T_%7B1%7D%29%2BL_%7Bf%7D%20%2B%20c_%7Bw%7D%5Ccdot%20%28T_%7B3%7D-T_%7B2%7D%29%5D)
(1)
Where:
- Mass of the sample, in grams.
- Specific heat of ice, in joules per gram-degree Celsius.
- Specific heat of water, in joules per gram-degree Celsius.
- Latent heat of fusion, in joules per gram.
- Initial temperature of the sample, in degrees Celsius.
- Melting point of water, in degrees Celsius.
- Final temperature of water, in degrees Celsius.
- Total energy, in joules.
If we know that 
, 
, 
, 
, 
, 
and 
, then the final energy to raise the temperature of the sample is:
![Q = (15\,g)\cdot \left[\left(2.06\,\frac{J}{g\cdot ^{\circ}C} \right)\cdot (5\,^{\circ}C)+ 334.72\,\frac{J}{g} + \left(4.184\,\frac{J}{g\cdot ^{\circ}C}\right)\cdot (35\,^{\circ}C) \right]](https://tex.z-dn.net/?f=Q%20%3D%20%2815%5C%2Cg%29%5Ccdot%20%5Cleft%5B%5Cleft%282.06%5C%2C%5Cfrac%7BJ%7D%7Bg%5Ccdot%20%5E%7B%5Ccirc%7DC%7D%20%5Cright%29%5Ccdot%20%285%5C%2C%5E%7B%5Ccirc%7DC%29%2B%20334.72%5C%2C%5Cfrac%7BJ%7D%7Bg%7D%20%2B%20%5Cleft%284.184%5C%2C%5Cfrac%7BJ%7D%7Bg%5Ccdot%20%5E%7B%5Ccirc%7DC%7D%5Cright%29%5Ccdot%20%2835%5C%2C%5E%7B%5Ccirc%7DC%29%20%5Cright%5D)
Hence, the correct answer is C.
