Total Energy to Heat Water Calculator:
Enter the values of mass of water, m(g), specific heat capacity of water, C(J/g.°C) and temperature change, ΔT(°C) to determine the value of Total energy, q(J).
Total Energy to Heat Water Formula:
The total energy required to heat water refers to the amount of thermal energy (heat) needed to raise the temperature of a given mass of water by a specific temperature difference. This energy is determined by the mass of the water, its specific heat capacity, and the temperature change it undergoes.
The specific heat capacity of water is a measure of how much energy is needed to raise the temperature of 1 gram of water by 1°C, typically expressed as 4.186J/g°C. The formula incorporates these variables to compute the total energy in joules or other units of energy.
This principle is fundamental in thermodynamics and has applications in industries like food processing, energy systems, and environmental science. Factors such as water purity and pressure can slightly affect its specific heat capacity. The formula assumes constant pressure and no phase changes, such as boiling or freezing, during the process.
The energy depends directly on the mass of water, the specific heat capacity and the temperature change. The relationship is linear; doubling any of the variables doubles the energy required.
Total energy, q(J) in Joules is equal to the product of the mass of water, m(g) in grams, the specific heat capacity of water, C(J/g.°C) in Joules per gram degree Celsius, and the temperature change, ΔT(°C) in degrees Celsius.
Total energy, q(J) = m(g)* C(J/g.°C) * ΔT(°C)
q(J) = total energy in Joules, J.
m(g) = mass of water in grams, g.
C(J/g.°C) = specific heat capacity of water in Joules per gram degree Celsius, J/g.°C(4.186J/g.°C).
ΔT(°C) = temperature difference in degree Celsius, °C.
Total Energy to Heat Water Calculation:
1.Find the energy required to heat 500 g of water from 25°C to 75°C.
Given: m(g) = 500g, C(J/g.°C) = 4.186J/g.°C, ΔT(°C) = 75 – 25 = 50°C.
Total energy, q(J) = m(g)* C(J/g.°C) * ΔT(°C)
q(J) = 500 * 4.186 * 50
q(J) = 104650J.
2.If 25,000 J of energy is used to heat water from 20°C to 40°C, find the mass of water.
Given: q(J) = 25000J, C(J/g.°C) = 4.186J/g.°C, ΔT(°C) = 40 – 20 = 20°C.
Total energy, q(J) = m(g)* C(J/g.°C) * ΔT(°C)
m(g) =q(J) / C(J/g.°C) * ΔT(°C)
m(g) = 25000 / 4.186 * 20
m(g) = 298.5g.