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

q=mcT

+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

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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)

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