Problem: 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 97.3 g water at 22.0°C. Calculate the final temperature of the metal and water mixture, assuming no heat loss to the surroundings.

🤓 Based on our data, we think this question is relevant for Professor Staff's class at UNL.

FREE Expert Solution

Step 1: Calculate the average specific heat of the metals:

Cave = CAlMass ratioAl + CFeMass ratioFeCave = (0.89Jg·°C)(5.00 g Fe15 g metal) + (0.45Jg·°C)(10.00 g Al15 g metal)

Cave = 0.60 J/g•°C


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Problem Details

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 97.3 g water at 22.0°C. Calculate the final temperature of the metal and water mixture, assuming no heat loss to the surroundings.

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What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Calorimetry concept. You can view video lessons to learn Calorimetry. Or if you need more Calorimetry practice, you can also practice Calorimetry practice problems.

What professor is this problem relevant for?

Based on our data, we think this problem is relevant for Professor Staff's class at UNL.

What textbook is this problem found in?

Our data indicates that this problem or a close variation was asked in Chemistry: An Atoms First Approach - Zumdahl 2nd Edition. You can also practice Chemistry: An Atoms First Approach - Zumdahl 2nd Edition practice problems.