When 0.1375 g of solid magnesium is burned in a constant-volume bomb calorimeter, the temperature increases by 1.126°c. the heat capacity of the bomb calorimeter, determined in a separate experiment, is 3024 j/°c. calculate the heat given off by the burning magnesium in kj/mol.

-24.76 kJ/mol

Explanation:

given,

mass of solid magnesium burned = 0.1375 g

the temperature increases by(ΔT) 1.126°C

heat capacity of of bomb calorimeter (C_{cal})= 3024 J/°C

heat absorbed by the calorimeter

heat released by the reaction

energy density will be equal to heat released by the reaction divided by the mass of magnesium

Energy density =

Energy density = -24.76 kJ/mol

heat given off by burning magnesium is equal to -24.76 kJ/mol

be subject to a force andchange its motion

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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.

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