If a 100.0 g sample of water at 60.0 c is added to a 100.0 g sample of water at 10.0 c determine the final temperature of water . assume no heat is lost to the surroundings

We can use the heat equation,
Q = mcΔT 

Where Q is the amount of energy transferred (J), m is the mass of the substance (kg), c is the specific heat (J g⁻¹ °C⁻¹) and ΔT is the temperature difference (°C).

Let's say
heat gained by 100.10 g of water at 10°C = Q₁
heat lost from 100.0 g of water at 60 °C = Q₂
Final temperature of the mixture = T

 Since, there is no heat is lost to the surroundings,
                                     Q₁ = Q₂
                        mc(T - 10) = mc(60 - T)
Since, m is same for both sides (100.0 g) and c is a constant for the water, we can cut off m and c from both sides. Then,
                              (T - 10) =(60 - T)
                                      2T = 60 + 10 
                                      2T = 70
                                        T = 35 °C

Hence, final temperature of water is T = 35 °C.

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All the elements are arranged by melting points on the periodic table. in row they go from metals to gasses. in the row from sodium to argon, sodium is more reactive than the one on its right, magnesium.