Chemistry, 04.02.2020 16:58 u8p4

If you combine 270.0 ml of water at 25.00 â°c and 100.0 ml of water at 95.0 â°c, what is the final temperature of the mixture? use 1.00 g/ml as the density of water.

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Answer from: hdamelis30

43.92 °C.

Explanation:

If we combine warm water with cold one, the heat will transfer from the hot water to the cold until reaching an equilibrium temperature.

The amount of heat released by hot water = the amount of heat absorbed by cold water.

The amount of heat released to or absorbed by water (Q) = m.c.ΔT.

where, Q is the amount of heat released to or absorbed by water.

m is the mass of water.

c is the specific heat capacity of water (c = 4.186 J/g.°C).

ΔT is the temperature difference (final T - initial T).

Since, d of water = 1.00 g/mL.

the mass of cold water at 25.0 °C = d.V = (1.00 g/mL)(270.0 mL) = 270.0 g.

the mass of warm water at 95.0 °C = d.V = (1.00 g/mL)(100.0 mL) = 100.0 g.

Q released by warm water = Q absorbed by cold water.

- (m.c.ΔT)released by warm water = (m.c.ΔT)absorbed by cold water.

Since c is the same so,

- (m.ΔT)released by warm water = (m.ΔT)absorbed by cold water.

- [(100 g)(final T - 95.0 °C)] = (270 g)(final T - 25.0 °C).

- 100 final T + 9500 = 270 final T - 6750.

270 final T + 100 final T = 9500 + 6750

370 final T = 16250.

∴ final T = 16250/370 = 43.92 °C.

Answer from: Quest

answer: c. the experiment shows that the red substance experienced a chemical change.

explanation: chemical change is the change in which chemical composition of the substance changes. physical change is the change in which there is no change in chemical composition.

chemical changes are accompanied by following changes:

a) precipitate formation

b) energy is released or absorbed

c) formation of bubbles

d) change in color

as it is given that the red color has disappeared and there is production of gas, it means the red substance has undergone a chemical change.

Answer from: Quest

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If you combine 270.0 ml of water at 25.00 â°c and 100.0 ml of water at 95.0 â°c, what is the final t...