Question

A student adds 45.00 grams of zinc metal (c_s = 0.377 J/g^oC) to 115.00 grams of water (c_s = 4.184 J/g^oC). 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?

Answer 1

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