To answer this, you need to know the ∆Hfusion of water, which happens to be 334 J/g. So, to melt 12.8 g of ice at 0ºC, the joules needed = (12.8 g)(334 J/g) = 4275 joules
The necessary heat is 4,27 joules.
In order to answer this question, you need the enthalpy of fusion of ice, which is 333.55 J/g (Joules/gram). The enthalpy of fusion is the amount of heat that must be absorbed or lost in order to change physical state. The number of Joules required to melt the ice = enthalpy of fusion of ice x mass of ice. Joules needed to melt the ice = 333.55 J/g x 40 g = 13342 J
how many calories are required to melt a 1.52g ice cube?
800kj-----------Apex<('-'<)
The energy required to melt a substance
125.6kj (apex)
This heat is 32,48 joules.
In order to answer this question, you need the enthalpy of fusion of ice, which is 333.55 J/g (Joules/gram). The enthalpy of fusion is the amount of heat that must be absorbed or lost in order to change physical state. The number of Joules required to melt the ice = enthalpy of fusion of ice x mass of ice. Joules needed to melt the ice = 333.55 J/g x 40 g = 13342 J
10,267 kJ are needed
In order to answer this question, you need the enthalpy of fusion of ice, which is 333.55 J/g (Joules/gram). The enthalpy of fusion is the amount of heat that must be absorbed or lost in order to change physical state. The number of Joules required to melt the ice = enthalpy of fusion of ice x mass of ice. 1 kg = 1000g 40kg x (1000g/1kg) = 40,000g Joules needed to melt the ice = 333.55 J/g x 40000 g = 13342000 J or 1.3342 x 107 J
2,26 Kj are necessary
Heat required to melt 1 g of ice at 0°C is approximately 80 cal . This is also called latent heat of fusion of ice.
226,ooo j
226,ooo j
how many calories are required to melt a 1.52g ice cube?
2.20X10to the 4
334 j/g =167000 j
334 j/g =167000 j