# Problem: A 4.96 g sample of gold, initially at 62.6˚C, is submerged into 55.1 g of ethanol at 20.1˚C in an insulated container. What is the final temperature of both substances at thermal equilibrium? (The specific heat capacity of gold is 0.128 J/g•˚C; the specific heat capacity of ethanol is 2.42 J/g•˚C)

###### FREE Expert Solution

$\overline{){\mathbf{q}}{\mathbf{=}}{\mathbf{mc}}{\mathbf{∆}}{\mathbf{T}}}$

+qabsorbs heat
–qloses heat

Heat transfer: hot to cold

heat released by gold = heat absorbed by ethanol

– qgold = + qethanol

At thermal equilibrium:

▪ final temperature of gold = final temperature of ethanol = final temperature of system

97% (404 ratings) ###### Problem Details

A 4.96 g sample of gold, initially at 62.6˚C, is submerged into 55.1 g of ethanol at 20.1˚C in an insulated container. What is the final temperature of both substances at thermal equilibrium? (The specific heat capacity of gold is 0.128 J/g•˚C; the specific heat capacity of ethanol is 2.42 J/g•˚C)