what number of joules needed to turn 325g of water at 100 degree c to steam at 100 degree c
q = (325 g)(2260 J/g)
*grams cancel out*
q = 734500 J
q = 7.345*10^5 J
Well, let's do some calculations and have a little fun with them! To turn water into steam, you need to consider two processes: heating the water to its boiling point and then converting it into steam.
First, we need to calculate the energy needed to heat the water from 100°C to its boiling point, which is 100°C. The specific heat capacity of water is approximately 4.18 J/g°C. So, to heat 325g of water by 1°C, we need 325g * 4.18 J/g°C = 1352.5 J.
Next, we need to calculate the energy needed for the phase change from liquid to gas, which is called the heat of vaporization. The heat of vaporization for water is approximately 2260 J/g. Therefore, to convert 325g of water into steam, we need 325g * 2260 J/g = 732,500 J.
Now we add those two values together: 1352.5 J + 732,500 J = 733,852.5 J.
So, approximately 733,852.5 Joules of energy are needed to turn 325g of water at 100°C into steam at 100°C. That's a lot of energy! Just like the energy I put into making you smile with my clownish answers!
To calculate the amount of energy (in joules) needed to convert a certain amount of water from its boiling point to steam at the same temperature, you need to consider two steps: raising the temperature of the water to its boiling point and then converting it to steam.
Step 1: Heating the water to its boiling point:
The specific heat capacity of water is 4.184 J/g°C.
First, calculate the energy required to heat water from 100°C to its boiling point:
Q1 = mass × specific heat capacity × change in temperature
Q1 = 325 g × 4.184 J/g°C × (100°C - 100°C)
Q1 = 0 J
Since the temperature difference is zero, no energy is required to heat the water to its boiling point.
Step 2: Converting water to steam:
The heat of vaporization for water is 2260 J/g.
Calculate the energy required to convert the water at its boiling point to steam:
Q2 = mass × heat of vaporization
Q2 = 325 g × 2260 J/g
Q2 = 732,500 J
Therefore, the total energy required to convert 325g of water at 100°C to steam at 100°C is 732,500 joules.
To calculate the number of joules required to convert a substance from one phase to another, we need to know the specific heat capacity and the heat of vaporization of the substance. For water, we also need to consider its change in temperature from 100°C as it transitions into steam.
Let's break down the steps to calculate the energy required to convert 325g of water at 100°C to steam at 100°C:
1. Calculate the energy required to raise the temperature of the water from 100°C to its boiling point, 100°C. The specific heat capacity of water is approximately 4.18 J/g°C. Since the temperature does not change, the equation to calculate this energy is:
Energy = mass × specific heat capacity × change in temperature
Energy = 325g × 4.18 J/g°C × 0°C = 0 joules
2. Once the water reaches its boiling point, energy is needed to convert the water at 100°C to steam at the same temperature. This energy is called the heat of vaporization of water. The heat of vaporization of water is approximately 2,260 J/g.
Energy = mass × heat of vaporization
Energy = 325g × 2,260 J/g = 733,250 joules
Therefore, the number of joules needed to turn 325g of water at 100°C to steam at 100°C is 733,250 joules.