If you combine 230.0 mL of water at 25.00 ∘ C and 140.0 mL of water at 95.00 ∘ C, what is the final temperature of the mixture? Use 1.00 g/mL as the density of water.

The final temperature of the mixture is 51.49°C

Explanation:

When two samples of water are mixed, the heat released by the water at high temperature will be equal to the amount of heat absorbed by water at low temperature

The equation used to calculate heat released or absorbed follows:

      ......(1)

where,

q = heat absorbed or released

= mass of water at high temperature = 140 g     (Density of water = 1.00 g/mL)

= mass of water at low temperature = 230 g

= final temperature = ?°C

= initial temperature of water at high temperature = 95.00°C

= initial temperature of water at low temperature = 25.00°C

c = specific heat of water= 4.186 J/g°C

Putting values in equation 1, we get:

Hence, the final temperature of the mixture is 51.49°C

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