Chemistry Calorimetry Solution: A 31.5 g wafer of pure gold initially at 69.7 oC i...

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# Solution: 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?

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?

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: View Complete Written Solution

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