How much heat is needed to convert 200 grams of ice at 0 degrees Celsius to steam at 100 degrees Celsius?(Hf(0 C)=334 J/g, Specific heat of water = 4.184 J/gK, Hv(100 C) = 2260 J/g, Specific heat of ice = 2.108 J/gC) and how do i do it?
In order to find out the energy needed to convert the phase of the water molecule from solid to gas form, one needs to calculate the energy consumed in each of the subsequent phase change. i.e From solid to liquid followed by from liquid to solid.
The summation of all the individual energies will result in the total energy required for the change seen.
How much heat is needed to convert 200 grams of ice at 0 degrees Celsius to...
How much heat (in kJ) is needed to convert 926 g of ice at −10.0°C to steam at 126.0°C? (The specific heats of ice, water, and steam are 2.03 J/g · °C, 4.184 J/g · °C, and 1.99 J/g · °C, respectively. The heat of fusion of water is 6.01 kJ/mol, the heat of vaporization is 40.79 kJ/mol
How much heat is needed to convert 0.75 kg of ice at -10 Celsius to steam at 120 Celsius?
Enter your answer in the provided box. How much heat (in kJ) is needed to convert 916 g of ice at -10.0°C to steam at 126.0°C? (The specific heats of ice, water, and steam are 2.03 J/g . oC, 4.184 J/g . oC, and 1.99 J/g , oC, respectively. The heat of fusion of water is 6.01 kJ/mol, the heat of vaporization is 40.79 k.J/mol.) k.J
How much heat required to convert 36 grams (2 moles) of ice at 0 degrees C to liquid water at 50 degrees C? delta-H of fusion for H2O is 6.02 kJ/mol and the heat capacity of liquid water is 4.18J/g degrees C. A) 12 kJ B) 7524 J C) 8728 J D) 19564 J
How much energy (heat) is required to convert 52.0 g of ice at -10.0 C to steam at 100 C?Specific heat of ice: 2.09 J/g * C DHfus = 6.02 kJ/molSpecific heat of water: 4.18 J/g * C DHvap = 40.7 kJ/molSpecific heat of steam: 1.84 J/g * C
William Lindsay What heat is needed to change the temperature of 5.2 grams ice fronm -10 C to water at 0 C? ut of Note: Cice 2.11 J/g C) oCwater 4.18J/g C) Csteam-2.08 J/(g"c) 120 100 Kvap 2260 J/g 80 Temperature (deg. C) 20 Kfus 334 J/g Energy Absorbed Answer Check
155 grams of ice at -10.0 degrees celsius is added to 1.17 kg of water at 70.0 degrees celsius and mixed together in thermal isolation until they come to equilibrium. The specific heat of ice is 2010 J/kgC. The specific heat of water is 4186 J/kgC. The latent heat of fusion for water is 3.34x10^5 J/kg. The latent of vaporization for water is 2.26x10^6 J/kg. What is the final equilibrium. The answer is 51.9 celsius. I just need the steps...
calculate how many J of heat should be added to convert 45.0 g of ice at -5.0 degrees celsius to steam at 100.0 degrees celsius
A 200 g piece of ice at 0 degrees Celsius is place in 500 g of water at 20 degrees Celsius. The system is in a container of negligible heat capacity and insulated from its surroundings. a) What is the final equilibrium temperature of the system? b) How much of the ice melts? The latent heat of fusion for water is (333.5 KI/kg). The specific heat of water is 4.18 KI/kg K Useful equations: Q = mlf and Q =...
How much heat is required to convert solid ice with a mass of 525 g and at a temperature of-23.5 °C to liquid water at a temperature of 48.5 °C? (The specific heat of ice is cice = 2100 /kgK, the specific heat of water is cwater-4186.8 J/kgK, and the heat of fusion for water is: Lf 334 kJ/kg.) Submit Answer Tries 0/12