Hi! I am having problems solving this question:
0.01kg of melting ice is put into a vacuum flask containing water with initial temperature 50.0'c.
The mixture is stirred well and the ice melts completely.
The final temperature of the water becomes 45.5'c. Assume that no energy is lost to the surrounding, what is the mass of the water originally in the flask?
(Specific heat capacity of water = 4200J/(kgK), specific latent heat of fusion of ice = 3.34x10^5)
ANS: 0.28kg
Anyone here knows how to solve this?
Originally posted by Okmijnub:Hi! I am having problems solving this question:
0.01kg of melting ice is put into a vacuum flask containing water with initial temperature 50.0'c.
The mixture is stirred well and the ice melts completely.
The final temperature of the water becomes 45.5'c. Assume that no energy is lost to the surrounding, what is the mass of the water originally in the flask?
(Specific heat capacity of water = 4200J/(kgK), specific latent heat of fusion of ice = 3.34x10^5)
ANS: 0.28kg
Anyone here knows how to solve this?
heat loss by water= heat gain by ice
Q = 0.01 x 4200x 45.5 + 0.01 x 3.34x10^5(( energy absorbed when ice melt to become water and heat absorbed by 45.5 deg)= A
A = M x 4200 x (50-45.5)
= 0.28kg
or thats how it should be done.