Question

In the laboratory, a student uses a coffee cup calorimeter to determine the specific heat of a metal. She heats 18.1 grams of lead to 99.50°C and then drops it into a cup containing 81.7 grams of water at 23.00°C. She measures the final temperature to be 23.67°C. Assuming that all of the heat is transferred to the water, she calculates the specific heat of lead to be _____ J/g°C.

Answer 1

`specificheat=0.177J/g^(0)C`

Step-by-step explanation:

The heat evolved by lead will be absorbed by water.

The heat evolved by lead will be:

`Q1=massXspecificheatXchangeintemperature`

`Q1=18.1X(Specificheat)X(99.50-23.67)`

Heat absorbed by water will be:

`Q2=massXspecificheatX(changeintemperature)`

`Q2=81.7X4.184(23.67-23)=229.03J`

We know that

Q1=Q2

`18.1X(Specificheat)X(99.50-23.67)=229.03`

`1372.523Xspecificheat=229.03`

`specificheat=0.177J/g^(0)C`