Compare the energy needed to raise the temperature of 1kg of water from 20°C to 100°C and the energy needed to boil 1kg of water at 100°C?
I turned 1kg to 1000g water is 4.18J/g°C and subtracted 20°C then i get confused as what to do next to
334400
To calculate the energy needed to raise the temperature of 1 kg (1000 g) of water from 20°C to 100°C, you can use the specific heat capacity of water, which is approximately 4.18 J/g°C.
The formula for calculating the energy needed to raise the temperature of a substance is:
Energy = mass × specific heat capacity × temperature change
For the first step, you would need to calculate the energy required to raise the temperature of the water from 20°C to 100°C:
Energy = 1000 g × 4.18 J/g°C × (100°C - 20°C)
Energy = 1000 g × 4.18 J/g°C × 80°C
Energy = 334,400 J
Therefore, the energy needed to raise the temperature of 1 kg of water from 20°C to 100°C is 334,400 Joules.
Now, to calculate the energy needed to boil 1 kg of water at 100°C, you will need to take into consideration the specific heat required to change water from liquid to gaseous state, which is known as the heat of vaporization. For water, the heat of vaporization is approximately 2260 J/g.
To find the energy needed to boil the water, use the formula:
Energy = mass × heat of vaporization
Energy = 1000 g × 2260 J/g
Energy = 2,260,000 J
Therefore, the energy needed to boil 1 kg of water at 100°C is 2,260,000 Joules.
To summarize:
- The energy required to raise the temperature of 1 kg of water from 20°C to 100°C is 334,400 Joules.
- The energy needed to boil 1 kg of water at 100°C is 2,260,000 Joules.
To compare the energy required to raise the temperature of 1kg of water from 20°C to 100°C and the energy needed to boil 1kg of water at 100°C, you need to consider two separate calculations.
1. Calculate the energy required to raise the temperature of 1kg (1000g) of water from 20°C to 100°C:
First, determine the temperature difference: 100°C - 20°C = 80°C.
Next, use the specific heat capacity of water, which is approximately 4.18 J/g°C, to calculate the energy required per gram.
Multiply the temperature difference by the mass of water and the specific heat capacity: 80°C * 1000g * 4.18 J/g°C = 334,400 J.
2. Calculate the energy required to boil 1kg (1000g) of water at 100°C:
The energy required to change the phase of a substance is given by its heat of vaporization. For water, this value is approximately 2,260 J/g.
Multiply the mass of water by the heat of vaporization: 1000g * 2260 J/g = 2,260,000 J.
Therefore, the energy needed to raise the temperature of 1kg of water from 20°C to 100°C is 334,400 J, while the energy needed to boil 1kg of water at 100°C is 2,260,000 J.
q1 = energy needed to raise T from 20 C to 100 C.
q1 = 1000g x 4.184 J/g*C x (100-20) = ?
q2 = heat needed to boil 1,000 g H2O at 100 C.
q2 = 1000 x heat vaporization in J/g = ?