# Problem: A 31.5 g wafer of pure gold initially at 69.7 oC is submerged into 63.6 g of water at 27.2 oC in an insulated container.What is the final temperature of both substances at thermal equilibrium?

###### FREE Expert Solution
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###### FREE Expert Solution

In this problem, we’re being asked to determine the final temperature of both the substances at thermal equilibrium.

Recall that heat can be calculated using the following equation:

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

q = heat, J

+qabsorbs heat
–qloses heat

m = mass (g)
c = specific heat capacity = J/(g·°C)
ΔT = Tf – Ti = (°C)

Recall that heat always travel from high-temperature object to lower-temperature object.

• In this problem, since the initial temperature of water lower than that of the initial temperature of gold, thus when they came in contact with each other, the heat from the gold would transfer into the water.

Based on the given system:

98% (430 ratings)
###### Problem Details

A 31.5 g wafer of pure gold initially at 69.7 oC is submerged into 63.6 g of water at 27.2 oC in an insulated container.

What is the final temperature of both substances at thermal equilibrium?

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 Thermal Equilibrium concept. You can view video lessons to learn Thermal Equilibrium Or if you need more Thermal Equilibrium practice, you can also practice Thermal Equilibrium practice problems .

How long does this problem take to solve?

Our expert Chemistry tutor, Dasha took 7 minutes to solve this problem. You can follow their steps in the video explanation above.

What professor is this problem relevant for?

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

What textbook is this problem found in?

Our data indicates that this problem or a close variation was asked in . You can also practice practice problems .