Step-by-step explanation:
How many joules are required to convert 325g of water at 12 degrees Celsius to steam at 176 degrees Celsius
To calculate the energy required to convert a given mass of water from a lower temperature to steam at a higher temperature, we need to consider two processes: (1) heating the water from its initial temperature to its boiling point, and (2) vaporizing the water at its boiling point to steam at the final temperature.
The amount of heat required for each process can be calculated separately using the following formulas:
(1) Q1 = m * c * ΔT
(2) Q2 = m * L
where Q1 is the heat required to raise the temperature of the water, Q2 is the heat required for the water to vaporize, m is the mass of water, c is the specific heat of water, ΔT is the temperature change, and L is the heat of vaporization of water.
Given:
Mass of water (m) = 325 g
Initial temperature of water = 12°C
Final temperature of steam = 176°C
Specific heat of water (c) = 4.184 J/g°C
Heat of vaporization of water (L) = 2260 J/g (at standard pressure)
To find the energy required to convert 325g of water at 12°C to steam at 176°C, we need to calculate Q1 and Q2 separately and then add them together.
(1) Heating the water:
Q1 = m * c * ΔT
Q1 = 325 g * 4.184 J/g°C * (100°C) [since the boiling point of water is 100°C at standard pressure]
Q1 = 136292 J
(2) Vaporizing the water:
Q2 = m * L
Q2 = 325 g * 2260 J/g
Q2 = 735500 J
Total heat required = Q1 + Q2
Total heat required = 136292 J + 735500 J
Total heat required = 871792 J
Therefore, it would require 871792 J of energy to convert 325g of water at 12°C to steam at 176°C.