Heat Problems. The specific heat of lead is 0.129 J/ g ° C . Find the amount of heat released when 497.28 g of lead are cooled from 37.2 ° C to 22.5 ° C.
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225.0 J of heat are applied to an 87.0 g sample of water. If the sample’s temperature was initially 18.9 °C , what will it’s final temperature be? The specific heat of water is 4.184J/g °C .
While taking a relaxing bubble bath one evening, Cindy wonders how much heat would be needed to convert a tub full of 50.5 L of water at 46.8 °C to steam at 100.0 °C. She knows that ΔHvap = 40.7kJ/mol for water and that Cwater = 4.184 J/g °C. Can you tell Cindy how much heat would be needed?
∆Hfus = 6.02 kJ/mol∆Hvap= 40.7 kJ/mol
What is the change in enthalpy when 17.50 mL of water at 60.00°C is converted to steam and heated to 112.00°C ?
∆Hfus = 6.02 kJ/mol, ∆Hvap = 40.7 kJ/mol1. What is the change in enthalpy when 32.00 g of ice at -5.00°C is converted to steam and heated to 122.00°C?
2. What is the change in enthalpy when 20.0 g of steam at 107°C is condensed into a liquid and cooled to 35°C?
3. What is the change in enthalpy when 85.0 g of water at 78°C freezes and cools to a solid at -