= 150 g x 4.184 J/g/K x (373 – 298) K = 47,070 J. Thus, 47,070 J are needed to increase the temperature of 150 g of water from 25 degrees C to its boiling point of 100 degrees C. One can follow a similar procedure to determine the energy needed to heat water from one temperature to another.

## How much energy is needed to boil 100g water?

The change in temperature is (100°C – 27°C) = 73°C. Since the specific heat of water is 4.18J/g/°C we can calculate the amount of energy needed by the expression below. Energy required = 4.18 J/g/°C X 100g X 73°C = 30.514KJ.

## How much energy is required to boil boiling water?

For water at its normal boiling point of 100 ºC, the heat of vaporization is 2260 J g^{–}^{1}. This means that to convert 1 g of water at 100 ºC to 1 g of steam at 100 ºC, 2260 J of heat must be absorbed by the water.

## How much energy does it take to boil a gram of water?

It takes 100 calories to heat 1 g. water from 0˚, the freezing point of water, to 100˚ C, the boiling point. However, 540 calories of energy are required to convert that 1 g of water at 100˚ C to 1 g of water vapor at 100˚ C. This is called the latent heat of vaporization.

## How much energy does it take to boil water calculator?

The specific heat capacity of water is 4.18 J/g/°C. We wish to determine the value of Q – the quantity of heat. To do so, we would use the equation Q = m•C•ΔT. The m and the C are known; the ΔT can be determined from the initial and final temperature.

## What is the total number of kilojoules required to boil 100 grams of water at 100?

Ernest Z. To convert 100.0 g of water at 20.0 °C to steam at 100.0 °C requires 259.5 kJ of energy.

## How much energy does it take to boil 100 mls of water if room temperature is 20C?

How much energy does it take to boil 100 mls of water if room temperature is 20c? From the steam tables, the heat capacity is close to 2 KJ/kg/deg C, far from 1.2 that you used, so it takes around 160 KJ to heat a kg of water to 100 C, from 20 C. This brings the total energy needed to 2418 KJ.

## How many kWh does it take to boil 1 Litre of water?

Based on the above answers and examples, to boil 1 litre of water from 20C to 100C, requiring 0.183 kWh of either electricity or gas, at todays energy prices GAS is 68% cheaper than electricity.

## Why is energy needed to boil water?

Boiling water is an endothermic process, which supplies heat to the water molecules, increasing their potential energy. … Once the intermolecular bonds are broken, any extra heat increases the kinetic energy of the system and the molecules of the water vapor move faster as the temperature increases.

## How many joules does it take to boil a kettle?

The power reading in watts is the energy in joules transferred electrically in one second by the heating element circuit. For the small kettle the rate is about 1,000 joules per second. For large the kettle it is close to 3,000 joules per second.

## What type of energy is boiling water?

Boiling water on a stove is an example of thermal energy. Thermal energy is produced when the atoms and molecules in a substance vibrate faster due to a rise in temperature.

## How much energy does it take to boil 100 mL of water apex?

So 100ml of water has a mass of 100 grams. The change in temperature is (100°C – 27°C) = 73°C. Since the specific heat of water is 4.18J/g/°C we can calculate the amount of energy needed by the expression below. Energy required = 4.18 J/g/°C X 100g X 73°C = 30.514KJ.

## How do you calculate the energy required to heat water?

Calculate the kilowatt-hours (kWh) required to heat the water using the following formula: Pt = (4.2 × L × T ) ÷ 3600. Pt is the power used to heat the water, in kWh. L is the number of liters of water that is being heated and T is the difference in temperature from what you started with, listed in degrees Celsius.