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## How much energy is required 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 does it take for water to boil?

The energy required to change water from a liquid to a solid is 333.7 kJ/kg while the energy required to boil water is 2257 kJ/kg. The amount of energy needed to change the phase of water to a gas from a liquid is 540 times the amount of energy needed to raise the same amount of water 1° C.

## How much energy does it take to boil 1g 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 is needed to evaporate 100g water?

The enthalpy of vaporization of water is 2256.4J/g, meaning that 2256.4J of heat are required to convert 1g of water at 100C to steam at 100C. In this case, we have 100g of water at 100C and we want to vaporize it to steam (also at 100C). This requires ΔH = 2256.4(100) = 225,640J or 225.64kJ of heat energy.

## What is the total KJ needed to completely boil 100.00 g of water at 100c?

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 much energy does it take to boil 1 Litre of water?

Again, heating of 1 litre of water from 20oC 100oC need 330kJ (0.091kWh) of heat. All these method provide the this amount of heat to water.

## How do you calculate water energy?

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.

## How do you calculate the energy needed 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.

## How much energy does it take to boil 1 kg of water?

Phase changes in pure water occur at a specific temperature. At 1 atm, water freezes at 0° C and boils at 100° C. The energy required to change water from a liquid to a solid is 333.7 kJ/kg while the energy required to boil water is 2257 kJ/kg.

## How many joules are required for boiling 21.1 g of water at 100 C?

For water at its normal boiling point of 100 ºC, the heat of vaporization is 2260 J g^{–}^{1}.

## How much energy does it take to vaporize 1 kg of water?

Even more energy is required to vaporize water; it would take 2256 kJ to change 1 kg of liquid water at the normal boiling point (100ºC at atmospheric pressure) to steam (water vapor).

## How much energy does it take to vaporize water?

Water has a heat of vaporization value of 40.65 kJ/mol. A considerable amount of heat energy (586 calories) is required to accomplish this change in water.

## What is the heat energy required to completely vaporize 10 grams of water?

What is the heat energy required to completely vaporize 10 text{ g}10 g of water beginning at 0°C? (The heat capacity of water is 4.2 J/g·K and the ? H_{vaporization} of water is 2260 kJ/kg) Choose 1 answer: (Choice A) 4.9 kJ (Choice B)