Explore BrainMass

Heat capacity

This content was STOLEN from BrainMass.com - View the original, and get the already-completed solution here!

A 5.00 g sample of aluminum pellets (specific heat capacity = 0.89 J/°C · g) and a 10.00 g sample of iron pellets (specific heat capacity = 0.45 J/°C · g) are heated to 100.0°C. The mixture of hot iron and aluminum is then dropped into 97.7 g of water at 24.2°C. Calculate the final temperature of the metal and water mixture, assuming no heat loss to the surroundings.

© BrainMass Inc. brainmass.com October 16, 2018, 4:10 pm ad1c9bdddf

Solution Preview

Heat given = Heat taken
<br>Let final temperature of metal+ water mixture be T degree C.
<br>Heat given by metal = m*c*Delta T = ...

Similar Posting

Description of Heat Capacity

Calculate the specific heat capacity of benzene(C6H6), given that 192 J of heat is required to raise the temperature of a 20.0g sample of benzene from 25.2 C to 38.8 C.

What is the molar heat capacity of benzene? (the molar heat capacity is the heat capacity of 1 mole of benzene)

3.50 Kcal of heat is removed from a 1.50 Kg sample of water initially at 25.2 C.
What is the final temperature?

Three separate experiments are done to determine the specific heat capacities of three different metals (zinc, platinum, and aluminium). The specific heat of each metal is determined as follows.

150.0 g of the metal initially at 100 Celsius is immersed in 50.0g of water initially at 22.0 Celsius. The final temperatures are given below. What is the specific heat capacity of each metal expressed as j/g Celsius?
a-Zinc, final temperature, 39.0 Celsius.
b- platinum, final temperature, 28.9 Celsius.
c-aluminium, final temperature, 52.8 Celsius.

View Full Posting Details