How much energy would it take to warm 30.0 g of water at 35 oC to the boiling point and boil all the liquid away?
To calculate the amount of energy required to heat and boil a substance, we need to consider two processes: heating the water from its initial temperature to the boiling point, and then supplying the latent heat of vaporization to convert the liquid to gas.
First, let's calculate the energy required to raise the temperature of the water from 35 °C to its boiling point (which is 100 °C at sea level):
1. Calculate the temperature difference:
ΔT = final temperature - initial temperature
ΔT = 100 °C - 35 °C = 65 °C
2. Apply the specific heat equation:
q1 = mass × specific heat × ΔT
q1 = 30.0 g × 4.18 J/g°C × 65 °C
Now, let's calculate the energy required to vaporize the water at its boiling point:
3. Apply the formula to calculate the heat of vaporization:
q2 = mass × heat of vaporization
q2 = 30.0 g × 2260 J/g (heat of vaporization for water)
Finally, we can calculate the total energy required:
Total energy = q1 + q2
Substituting the values:
Total energy = (30.0 g × 4.18 J/g°C × 65 °C) + (30.0 g × 2260 J/g)
Calculate the final result to find the total energy required.
Q=mc(final T- initial T)
final T=100 oC (boiling point)
http://www.ausetute.com.au/heatcapa.html