how much heat is needed to convert 8.75g of 100c water to steam?
q = mass water x deltaHvap.
To calculate the amount of heat required to convert water to steam, you need to use the formula:
q = m × ∆H
Where:
q is the amount of heat energy (in joules) required,
m is the mass of the substance (in grams), and
∆H is the heat of vaporization (in joules/gram)
In this case, you have 8.75 grams of water that needs to be converted to steam.
First, you will need to determine the ∆H value for water, which is the heat of vaporization. The heat of vaporization of water is approximately 40.7 kJ/mol, or 40.7 J/g.
So ∆H for converting water to steam is 40.7 J/g.
Now, you can calculate the heat energy required:
q = m × ∆H
q = 8.75 g × 40.7 J/g
By multiplying the mass of water (8.75 g) by the heat of vaporization (40.7 J/g), you can determine the amount of heat energy required to convert 8.75 grams of water to steam.
Performing the calculation:
q = 355.63 J
Therefore, approximately 355.63 Joules of heat energy is needed to convert 8.75 grams of 100°C water to steam.