Calculate the total amount of energy required to change 10.0 g of water from 35.0 degrees Celsius to 110. degrees Celsius.

The total amount of energy required is 25,515.2 J.

Explanation:

Calorimetry is the measurement and calculation of the amounts of heat exchanged by a body or a system.

When a system absorbs (or gives up) a certain amount of heat, it can happen that:

To calculate the latent heat the formula is used:

Q = m. L

Where

To calculate sensible heat the following formula is used:

Q = m. c. ΔT

where:

In this case, you have in the first place a heat to raise the temp of the water from 35.0 C to 100 C, where the specific heat value for water is  4.184 :

q1 = m*c*(Tfinal-Tinitial)

q1 = 10.0 g *(4.184 )* (100 - 35.0 C) = 2719.6 J

Now you have the heat to vaporize the water, where the heat of vaporization is 2259.36 :

q2 = m*(heat of vaporization)

q2 = 10.0 g*(2259.36 ) = 22593.6 J

Finally, you have the heat to raise temp of steam to 110 C, where the specific heat value for steam is  2.02 :

q3 = m*c*(Tfinal-Tinitial)

q3 = 10.0 g*(2.02 )*(110-100 C) = 202 J

The total amount of energy can be calculated as:

Q= q1 + q2 + q3

Q= 2719.6 J + 22593.6 J + 202 J

Q=25,515.2 J

The total amount of energy required is 25,515.2 J.

chemistry sucks a**

explanation:

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