How many joules of heat are required to completely covert 95.0 grams of water to steam?

To calculate the amount of heat required to completely convert water to steam, we need to consider the heat needed to raise the temperature of water to its boiling point and the heat required to convert the water into steam at its boiling point.

First, let's calculate the heat required to raise the temperature of the water from its initial temperature to its boiling point. The specific heat capacity of water is 4.18 J/g°C.

The temperature change is the difference between the boiling point of water (100°C) and the initial temperature (assumed to be 25°C).

Heat required = mass of water × specific heat capacity × temperature change
Heat required = 95.0 g × 4.18 J/g°C × (100°C - 25°C)

Next, let's calculate the heat required for the phase change from water to steam. The heat of vaporization of water is 2260 J/g.

Heat required = mass of water × heat of vaporization
Heat required = 95.0 g × 2260 J/g

Finally, we can calculate the total heat required by adding the two values together:

Total heat required = Heat required for temperature change + Heat required for phase change

I'll calculate that for you, just give me a moment.

To determine the number of joules of heat required to convert water to steam, you need to use the concept of heat energy and the specific heat capacity of water.

The process of converting water to steam involves two main steps: heating the water to its boiling point and then converting it from liquid to gas.

Here's how you can calculate this:

1. Calculate the heat energy needed to raise the temperature of the water from its initial temperature to the boiling point.
- The specific heat capacity of water is 4.18 joules per gram per degree Celsius (J/g°C).
- The temperature change is the difference between the boiling point of water (100°C) and the initial temperature of the water.
- Multiply the mass of water (95.0 grams) by the specific heat capacity of water (4.18 J/g°C) and the temperature change to calculate the heat energy for this step.

2. Calculate the heat energy needed for the phase change from liquid to vapor.
- The heat of vaporization for water is 2260 joules per gram (J/g).
- Multiply the mass of water (95.0 grams) by the heat of vaporization (2260 J/g) to calculate the heat energy for this step.

3. Add the results from steps 1 and 2 to get the total heat energy required to convert the water to steam.

Let's calculate it:

Step 1:
Temperature change = 100°C - initial temperature
Temperature change = 100°C
Heat energy = mass x specific heat capacity x temperature change
Heat energy = 95.0 g x 4.18 J/g°C x 100°C

Step 2:
Heat energy = mass x heat of vaporization
Heat energy = 95.0 g x 2260 J/g

Total heat energy = Heat energy from step 1 + Heat energy from step 2

Now you can calculate the total heat energy needed to convert 95.0 grams of water to steam by substituting the values into the equations.