If you have 0.341 m3 of water at 25.0 ∘C in an insulated container and add 0.127 m3 of water at 95.0 ∘C, what is the final temperature f of the mixture? Use 1000 kg/m3 as the density of water at any temperature.

Explanation:

Hello!

In this case, since this calorimetry problem is about the mixing of two volumes of water, we can infer that the heat lost by the hot water is gained by the cold water so we can write:

Which in terms of mass, specific heat and temperature change is:

Clearly, the specific heat is the same for both waters and the masses, considering the given densities are:

Thus, we can solve for the the final temperature as shown below:

And by plugging in the values we obtain:

Best regards!

1. a)c-14 has two more protons

2. d)they have different numbers of protons, neutrons, and valence electrons; they are all gases at room temperature.

3. c) iron and nickel.