How much energy (in kJ) does it take to heat 1000L of water from 15 degrees * C to 25 degrees * C ?​

Heat Q is the thermal energy transferred from a hotter system to a cooler system that are in contact.

Q=m.Cp.ΔT (Eq.1)

The equation above relates the temperature or the temperature difference of a substance or fluid with the thermal energy required to transfer Heat (whether heating or cooling).

Temperature is a measure of the average kinetic energy of the atoms or molecules in the system.

The thermal energy Q is calculated by the product of the mass of the substance (kg) by the specific heat of the substance or fluid (kJ/kg.k) by the temperature difference ΔT (.K) in degrees Kelvin.

Example: Heat output required to heat up 1000 litres of water from 5.C to 18.C (degrees Celsius).

Q=m.Cp.ΔT

Q = ~ 54,7kW

explanation:

let the different atoms be x and y. each with four protons and same mass will be represented as follows.

mass number is number of protons + number of neutrons.

            and  

since, it is given that one has a negative charge while the other is neutral. therefore, there will be increase in number of protons and the atom will be represented as follows.

according to periodic table, mass number of beryllium is 9 and it has atomic number 4 so, the atoms will be and .  

the protons and neutrons will be located inside the nucleus whereas the electrons will be revolving around the nucleus.