How much heat should be taken from 5 g of water at 0oc to transform it completely into ice?

Heat required to melt 5g of ice at 0°C to water at 0°C = 5g × 80 calorie per gram= 400 calorie.

How many calories does it take to change 1g of ice at 0 degrees Celsius to steam?

The ice temperature must be raised 10 degrees to reach 0oC. Since the specific heat of ice is 0.50 cal/g-oC, that means that 0.50 calories is needed to raise 1g of ice 1oC.

How many calories does it take to heat 10 grams of ice at 0oc to 50 OC water?

So,to convert 10g of ice at 0∘C to same amount of water at the same temperature, heat energy required would be 80⋅10=800 calories.

How do you calculate kcal of heat?

Specific Heat

1. For a mass m = gm = kg.
2. with specific heat c = cal/gm°C = joule/gm°C,
3. initial temperature Ti = °C = K = °F.
4. and final temperature Tf = °C = K = °F,
5. Q = calories = kcal = x 10^ calories.
6. Q = joules = x 10^ joules.

How many calories of heat are required to change 1 gram of ice at 0 C to liquid water at 0 C?

80 calories
– To melt 1 gram of ice requires 80 calories. (A calorie is defined as the amount of energy needed to raise one gram of water 1°C.)

How do you calculate heat change?

Subtract the final and initial temperature to get the change in temperature (ΔT). Multiply the change in temperature with the mass of the sample. Divide the heat supplied/energy with the product. The formula is C = Q / (ΔT ⨉ m) .

How many calories does it take to heat 10 grams of ice to 20 degrees C?

Explanation: When 10g of ice at −20°C s being converted into steam at 100°C , there are four stages. Ice at −20°C to ice at 0°C – here it continues to be in the same state i.e. ice and hence heat required is mass×specific heat×change in temperature Specific heat for ice is 0.5 cal/g-°C.

How much heat is gained by the water?

What is the specific heat capacity value of water? The specific heat of water is 4179 J/kg K, the amount of heat required to raise the temperature of 1 g of water by 1 Kelvin.

What is the specific heat of steam and ice?

specific heat of ice = 2.09 J/g·°C. specific heat of water = 4.18 J/g·°C. specific heat of steam = 2.09 J/g·°C. Solution: The total energy required is the sum of the energy to heat the -10 °C ice to 0 °C ice, melting the 0 °C ice into 0 °C water, heating the water to 100 °C, converting 100 °C water to 100 °C steam and heating the steam to 150 °C.

How do you calculate the total energy required to heat ice?

The total energy required is the sum of the energy to heat the -10 °C ice to 0 °C ice, melting the 0 °C ice into 0 °C water, heating the water to 100 °C, converting 100 °C water to 100 °C steam and heating the steam to 150 °C. To get the final value, first calculate the individual energy values and then add them up.

How many joules are in a gram of ice?

It is 1 calorie/gram °C = 4.186 joule/gram °C and is higher than any other common substance. On the other hand, the Heat required to raise the temperature of ice from 0°C to water at 10 °C is 90 calories, that is 9 times the Heat required to raise the temperature of water at 0°C to water at 10°C , or 376.56 Joules.

How many calories does it take to melt 1g of ice?

If 1 g of water is given 2 calories of heat , its temperature (of water) will go up by 2°C degrees. It takes 80 calories to melt 1 gram of ice. This is called Latent heat of melting of ice.

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