It requires 1 calorie to increase 1 mL of water by 1 degree Celsius. In 68 grams of water, there are 68 mL. The change in temperature is 7 degrees, so 476 calories are needed. 1 calorie has 4.184 joules, hence 1.992 kJ are needed.
19.7 kJ
5x2260, so 11,300 J or 11.3 KJ
The simple beginning is that the definition of a calorie is "the energy required to raise the temperature of 1g of water 1°C." Therefore, the energy required to raise 17g of water 32°C: 17*32=544 cal. However, the question asked about ice. There is an extra bit of energy required for the change of physical state. The energy required to convert 1 gram of ice at 0°C to liquid water at 0°C is called the "latent heat" and is equal to about 80 cal. To convert 17g of ice, we multiply this together: 17g * 80cal/g = 1360 cal. So, we add this energy required for the change of state to the energy required to raise the listed quantity to the required temperature and we get 544 cal + 1360 cal = 1904 cal, assuming no heat is lost to the environment. I hope this clarifies some things.
Lets say, for example the enthalpy is equal to 1200 joules/gram. You take 1200 joules/gram * (# of grams)/one mole [now you can cancel grams and it is now joules/mole.] Then convert the answer to kilojoules by dividing by 1000.
The energy required to completely separate the molecules in a liquid and convert them to a gas (boiling), is greater than the energy needed to completely separate the molecules in a solid and convert them to a liquid (melting).
7.9
19.7 kJ
Assuming standard atmospheric pressure, 2260 kilojoules.
5x2260, so 11,300 J or 11.3 KJ
The density of water @ 100oC (boiling point) is about 0.958 g/ml. First we need to convert the 155 ml to mass by multiply by the density.155 ml * (0.958 g/ml) = 148.49 gramsNext convert the grams to moles by dividing by the molecular weight of water, which is 18 g/mol:148.49 grams /(18 g/mol) = 8.25 mol of H2OFinally multiply the moles of water by the heat of vaporization (Hvap) to get the final answer:8.25 mol * (40.7 kJ/mol) = 335.775 kJ
It has been found that 4.2 kilojoules of energy raises the temperature of 1000g of water by 1•c.
It would depend on the temperature of the water, or average kinetic energy. (KE) However, what you may be looking for is how much heat is needed to raise the KE, or temperature, of water. 4.184 kilojoules per gram is the heat required to raise the temperature of water 1 degree Celsius.
If you mean hydraulic energy, you don't really "convert water to energy". If the water is in a higher position, it has more energy (potential energy); when it falls down, this potential energy is converted to some other type of energy.
The simple beginning is that the definition of a calorie is "the energy required to raise the temperature of 1g of water 1°C." Therefore, the energy required to raise 17g of water 32°C: 17*32=544 cal. However, the question asked about ice. There is an extra bit of energy required for the change of physical state. The energy required to convert 1 gram of ice at 0°C to liquid water at 0°C is called the "latent heat" and is equal to about 80 cal. To convert 17g of ice, we multiply this together: 17g * 80cal/g = 1360 cal. So, we add this energy required for the change of state to the energy required to raise the listed quantity to the required temperature and we get 544 cal + 1360 cal = 1904 cal, assuming no heat is lost to the environment. I hope this clarifies some things.
Lets say, for example the enthalpy is equal to 1200 joules/gram. You take 1200 joules/gram * (# of grams)/one mole [now you can cancel grams and it is now joules/mole.] Then convert the answer to kilojoules by dividing by 1000.
3
We can convert electrical energy into mechanical energy in mixer and grinder. We can convert electrical energy into sound energy in various sound systems. We can convert electrical energy into heat energy in electric water or room heater.