# What is the final temperature of the copper and water given that the specific heat of copper is 0.385 #J/(g * "^oC)#?

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A hot lump of 48.7 g of copper at an initial temperature of 76.8 C is placed in 50.0 mL of #H_2O# initially at 25.0°C and allowed to reach thermal equilibrium. Assume no heat is lost to surroundings.

A hot lump of 48.7 g of copper at an initial temperature of 76.8 C is placed in 50.0 mL of

##### 1 Answer

#### Explanation:

Here, we're setting the heat values derived given the equation:

equal to each other, as such,

Before we start, I will assume the density of water is