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.
Molar mass of H2O,
MM = 2*MM(H) + 1*MM(O)
= 2*1.008 + 1*16.0
= 18.016 g/mol
mass(H2O)= 9.00 g
use:
number of mol of H2O,
n = mass of H2O/molar mass of H2O
=(9 g)/(18.02 g/mol)
= 0.4996 mol
For condensation,
Q = -Hvap * number of mol
= -40.66 KJ/mol * 0.4996 mol
= -20.3 KJ
Answer: 20.3 KJ RELEASED
Calculate the heat that is absorbed/released when 9.00 g of steam condenses to liquid water at...
the heat of vaporization of water at 100*c is 40.66 kj/mol. calculate the quantity of heat that is absorbed/released when 9.00 g of steam condenses to liquid water at 100*c
The heat of vaporization of water at 100°C is 40.66 kJ/mol. Calculate the quantity of heat that is absorbed/released when 5.00 g of steam condenses to liquid water at 100°C. 147 kJ of heat are absorbed. 147 kJ of heat are released. 11.3 kJ of heat are absorbed 11.3 kJ of heat are released.
When steam condenses, is heat absorbed (endothermic) or released (exothermic)? When water freezes, is heat absorbed or released? Explain your reasoning.
The heat of vaporization of water at 100°C is 46.06 kJ/mol. Calculate the quantity of heat that is absorbed/released when 90.0 g of steam condenses to liquid water at 100°C. 203 kJ of heat are absorbed. 20.3 kJ of heat are released. 230.3 kJ of heat are released. 203.3 kJ of heat are released.
the heat of vaporization of water at 100C is 2.26kj/g. calculate the quantity of heat and specify if heat is absorbed or released when 9.00 g of steam condenses to liquid water at 100C
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 amount of heat that must be absorbed by 100.0 g of water at 20.0°C to convert it to steam (water vapor) at 110.0°C. Given: Specific heats: (liq) = 4.18 J/g·°C (steam) = 1.84 J/g·°C DHvap = 40.7 kJ/mol
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 liquid water and then cools to 28.00 °C.
how much heat is released when 10.0 g of steam (water vapor ) at 105.0 C is cooled to liquid water at 25 C? S(water) = 4.18 J/g.C. ... S(steam) = 2.01 j/ g.C the heat of fusion of water is 6.02 KJ/ mol. The heat of vaporization of water is 40.7 KJ/mol