how many calories are released when 100. g of steam condenses?

Question

Question

Answer 1

Answer #1

1g of water convert to steam is observe 540 calories.

So the reverse process,the 1g of steam convert to water is released 540 calories.

In this way 100g of water condense means

released calories =540×100

=54000 calories (or)54 kcalories

Answer 2

Similar Homework Help Questions

Calculate the energy released when 50.0g of steam condenses at 100℃.

Calculate the energy released when 50.0g of steam condenses at 100℃.Use the cooling curve to show what happens when 50.0g steam condenses at 100℃ and then cools to 20℃. Then calculate this energy change.6. Use the below cooling curve for water for the following questions. A. Label the melting/freezing point. B. Label the boiling/evaporation point. C. At what state is water when the temperature is 80 °c? D. At what state is water when the temperature is -20 °C? E. What happens to the temperature...
Calculate the heat that is absorbed/released when 9.00 g of steam condenses to liquid water at...

Calculate the heat that is absorbed/released when 9.00 g of steam condenses to liquid water at 100°C. DHvap(water) = 40.66 kJ/mol.
When steam condenses, is heat absorbed (endothermic) or released (exothermic)? When water freezes, is heat absorbed...

When steam condenses, is heat absorbed (endothermic) or released (exothermic)? When water freezes, is heat absorbed or released? Explain your reasoning.

In an insulated container, a mass m of steam at 100 ℃ condenses in 620 g...

In an insulated container, a mass m of steam at 100 ℃ condenses in 620 g of alcohol and then cools down, heating the alcohol from 20 ℃ to the final mixture temperature of 40 ℃? What is m? [Steam’s Latent heat of condensation is 540 cal/g; alcohol’s ca= .581 cal/(g * ℃) waters cw=1.00 cal/(g * ℃)]
Calculate the change in heat when 12.50 g of water vapor (steam) at 100.0°C condenses to...

Calculate the change in heat when 12.50 g of water vapor (steam) at 100.0°C condenses to liquid water and then cools to 22.00 °C.
Calculate the change in heat when 22.00 g of water vapor (steam) at 100.0°C condenses to...

Calculate the change in heat when 22.00 g of water vapor (steam) at 100.0°C condenses to liquid water and then cools to 28.00 °C.

If the specific heat of ethanol is 0.588, how many calories are released when 35.5 grams...

If the specific heat of ethanol is 0.588, how many calories are released when 35.5 grams of ethanol is heated from 65.5 degrees Celcius to 101 degrees Celcius?
How many calories needed to to boil 1250 g of water at 100°C

How many calories needed to to boil 1250 g of water at 100°C
Calculate how many grams of ice at 0°C would be melted by 100 g of 100°C...

Calculate how many grams of ice at 0°C would be melted by 100 g of 100°C steam. Hint: heat will be transferred from the steam to the ice in two processes: •the steam will condense into liquid, and •that liquid will transfer heat until it is at the freezing point of water. Note that for water: Lf = 80 cal/g (ice), and Lv = 540 cal/g (steam) (Use calories) C(water) =1 cal/g*C Answer in grams no decimal places.

A. Calculate the heat change in calories for condensation of 12.0 gg of steam at 100∘C...

A. Calculate the heat change in calories for condensation of 12.0 gg of steam at 100∘C Is it absorbed or released? B. Calculate the heat change in joules for condensation of 7.10 gg of steam at 100∘C∘C. Express your answer as a positive value using three significant figures and include the appropriate units. Is it absorbed or released? C. Calculate the heat change in kilocalories for vaporization of 45 gg of water at 100∘C∘C. Express your answer as a positive...