The latent heat of vaporization of water is #2260# #J##/##g#. How many kilojoules per gram is this, and how many grams of water will vaporized by the addition of #2.260*10^3# #J# of heat energy at #100°C#?
The latent heat of vaporization for a given substance indicates the amount of energy required for one mole of that substance to undergo a phase change, or transition from liquid to gas, at its boiling point.
As an alternative to the more widely used kilojoules per mole, the latent heat of vaporization for water in your situation is expressed in Joules per gram.
Therefore, you must calculate the number of kilojoules per gram needed to enable the transition from liquid to vapor in a given sample of water at its boiling point.
As you are aware, there is a conversion factor between joules and kilojoules that is
Here's the second portion of the query. As you are aware,
which implies that
This is the latent heat of vaporization per gram of water, meaning that one gram of water will vaporize at its boiling point when that much heat is applied to a sample of water.
By signing up, you agree to our Terms of Service and Privacy Policy
The latent heat of vaporization of water is 2.26 kJ/g. To calculate the grams of water vaporized by the addition of 2.26 kJ of heat energy at 100°C, divide the heat energy by the latent heat of vaporization: ( \frac{2.26 , kJ}{2.26 , kJ/g} = 1 , g ). Therefore, 1 gram of water will vaporize.
By signing up, you agree to our Terms of Service and Privacy Policy
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
- What is the difference between standard enthalpy of combustion and standard enthalpy of formation?
- Can you go over #q = m * c * DeltaT# ?
- A35.8 g sample of cadmium metal was melted by an electric heater providing 4.66 J/s of heat. If it took 6.92 min from the time the metal began to melt until it was completely melted, what is the heat of fusion per mole of cadmium?
- How can I calculate enthalpy of combustion?
- In a experiment it is observed that 252 J of heat must be absorbed to raise the temperature of 50.0 g of Ni(s) from 20.0 C to 31.4 C. How do you calculate the specific heat of Ni in both J/g °C and cal/g.C?

- 98% accuracy study help
- Covers math, physics, chemistry, biology, and more
- Step-by-step, in-depth guides
- Readily available 24/7