A chemist heats 37.35 g of lead to 67.71 °C , then places the metal sample in the cup of water shown in the interactive. Calculate the final temperature of the water. The specific heat of lead is 0.130 J/g⋅°C and the specific heat of water is 4.184 J/g⋅°C . mass of water: 60.000g
initial temperature of water: 25.00 C

Explanation:

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In this case, since the calorimetry problems involving how the heat released by a hot substance is gained by the cold substance when they are placed in contact until they reach the thermal equilibrium is mathematically defined via:

In this problem, it is seen that the lead is hot and the water cold, so we can write:

Thus, since it is asked for the final temperature, or equilibrium temperature, we solve for it as shown below:

Then, by plugging in the known data we obtain:

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every chemical equation adheres to the law of conservation of mass, which states that matter cannot be created or destroyed. therefore, there must be the same number of atoms of each element on each side of a chemical equation.

b) nuclear ive learned that in a pedtrodic table