A student adds 45.00 grams of zinc metal (cs = 0.377 J/goC) to 115.00 grams of water (cs = 4.184 J/goC). The initial temperature of the metal is 98.00 oC and the initial temperature of the water is 21.00 oC. What is the final temperature of the metal and water?
m(water) = 115.0 g
T(water) = 21.0 oC
C(water) = 4.184 J/goC
m(metal) = 45.0 g
T(metal) = 98.0 oC
C(metal) = 0.377 J/goC
T = 21.4 oC
We will be using heat conservation equation
Let the final temperature be T oC
use:
heat lost by metal = heat gained by water
m(metal)*C(metal)*(T(metal)-T) = m(water)*C(water)*(T-T(water))
45.0*0.377*(98.0-T) = 115.0*4.184*(T-21.0)
16.965*(98.0-T) = 481.16*(T-21.0)
1662.57 - 16.965*T = 481.16*T - 10104.36
T= 23.6224 oC
Answer: 23.62 oC
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