If you combine 230.0 mL 230.0 mL of water at 25.00 ∘ C 25.00 ∘C and 120.0 mL 120.0 mL of water at 95.00 ∘ C, 95.00 ∘C, what is the final temperature of the mixture? Use 1.00 g/mL as the density of wate

The final temperature of the mixture is  49°C

Explanation:

To calculate the mass of water, we use the equation:

For cold water:

Density of cold water = 1 g/mL

Volume of cold water = 230.0 mL

Putting values in above equation, we get:

For hot water:

Density of hot water = 1 g/mL

Volume of hot water = 120.0 mL

Putting values in above equation, we get:

When hot water is mixed with cold water, the amount of heat released by hot water will be equal to the amount of heat absorbed by cold water.

The equation used to calculate heat released or absorbed follows:

     ......(1)

where,

q = heat absorbed or released

= mass of hot water = 120 g

= mass of cold water = 230 g

= final temperature = ?°C

= initial temperature of hot water = 95°C

= initial temperature of cold water = 25°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  49°C

1.from liquid state to gaseous state is evaporation 3.solid to liquid is melting 5. solid to gaseous state is sublimation 6. gas to solid state is decomposition 7. a change of state is known as the states of matters

Sorry i dont understand the question can you rephase it?