The ice must be warmed with 4.719 kJ of heat.
How do you calculate heat to melt ice?
- Let's have a look at the energy required to melt one kilogramme of ice at absolute zero to create one kilogramme of water at absolute zero.
- We determine that Q = mLf = (1.0 kg)(334 kJ/kg) = 334 kJ is the energy required to melt a kilogramme of ice using the equation for a change in temperature and the value for water from Table 1.
- The quantity of heat energy required to transform materials from a solid to a liquid is known as the heat of fusion (melting.)
- The heat of fusion calculation formula is q = mHf.
- 2090 Joules/kg C is the specific heat of ice.
Given data :
- The mass of ice is, m = 10.0 g.
- The initial temperature is, T = - 10 degree Celsius.
- The final temperature is, T' = 110.0 degree Celsius.
- The heat capacity of ice is, c = 2.09 J/g C.
- The heat capacity of steam is, c' = 2.01 J/g C.
When ice absorbs heat, the conversion takes place from ice to water (liquid) and from the liquid to steam at 110 degree Celsius. So,
The amount of heat absorbed is given as,
Q = m[c(T' - T) + c'T']
Q = 10 [ 2.09 ( 110 - ( -10) + ( 2.01 x 110) ]
Q = 4719 J
Convert in kJ as,
Q = 4719/1000
Q = 4.719 kJ
Thus, we can conclude that the amount of heat required to warm the ice is 4.719 kJ.
Learn more about calculate heat to melt ice refer to :
https://brainly.com/question/26549639
#SPJ4
