Question

1. One litre of water at 30" C is mixed with one litre of water at 50" C.​

Answer 1

Answer:

the temperature will slightly less than 40°C. Explanation: Because water expands when heated, 1 litre of water at 50°C will have less mass than 1 litre of water at 30°C. As a result, the 30°C litre has slightly more than the 50°C litre, and thus the average will end up slightly less than 40°C.

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Answer 2

Answer:

Let the first volume of water be V1. Let the second volume of water be V2. Let the initial temperature of the first volume of water be θ1. Let the initial temperature of the second volume of water be θ2.

Let the energy required to heat a unit volume of water by unit temperature by C.

So, if the final temperature is θfinal, we have

heat gained by the first volume of water

=V1×C×(θfinal−θ1)

and

heat lost by the second volume of water

=V2×C×(θ2−θfinal).

By the law of conservation of energy,

heat lost = heat gained

∴V1×C×(θfinal−θ1)=V2×C×(θ2−θfinal)

∴V1θfinal−V1θ1=V2θ2−V2θfinal

∴θfinal=V1θ1+V2θ2V1+V2

Substituting the given values,

θfinal=230+50

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