Question

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

Answer 1

Answer:

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:

• experience a change in its temperature, which involves sensible heat,
• undergoes a phase change at constant temperature, or latent heat.

To calculate the latent heat the formula is used:

Q = m. L

Where

• Q: amount of heat
• m: mass
• L: latent heat

To calculate sensible heat the following formula is used:

Q = m. c. ΔT

where:

• Q: amount of sensible heat  
• m: body mass
• c: specific heat of the substance
• ΔT: temperature range

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 $\frac{J}{g*C}$:

q1 = m*c*(Tfinal-Tinitial)

q1 = 10.0 g *(4.184 $\frac{J}{g*C}$)* (100 - 35.0 C) = 2719.6 J

Now you have the heat to vaporize the water, where the heat of vaporization is 2259.36 $\frac{J}{g}$:

q2 = m*(heat of vaporization)

q2 = 10.0 g*(2259.36 $\frac{J}{g}$) = 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 $\frac{J}{g*C}$ :

q3 = m*c*(Tfinal-Tinitial)

q3 = 10.0 g*(2.02 $\frac{J}{g*C}$)*(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.