How much heat is required to warm 1.40 l of water from 20.0 ∘c to 100.0 ∘c? (assume a density of 1.0g/ml for the

The heat required to warm 1.40 l of water from 20.0 °C to 100.0 °C is 468.608 KJ.

Given to us

We know that the specific heat of the water is equal to  4184 J⋅kg−1⋅K−1.

We know  heat can be written as,

Substitute the values,

Hence, the heat required to warm 1.40 l of water from 20.0 ∘c to 100.0 ∘c is 468.608 KJ.

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hello, i am papaguy.

i have found an answer to your question but use it as information.

information: because weak acids/bases have low concentration of hydrogen ions, the addition of water has a large impact on the ph. 2. a difference in 1 unit is a 10x difference in concentration for example; a liquid with ph of 3 is 10x more acidic than a liquid with a ph of 4. therefore, a liquid with a ph of 3 is stronger.

best of luck!

connect the batteries in series and hope