The combustion of 10.0 g of an unknown chemical with molar mass = 35.56 g/mol, raises the temperature of 600 mL of water by 25oC. Assuming all the energy released by the reaction is absorbed only by the water, determine the ∆Hcomb of Mg. Note: specific heat capacity H20 = 4.18 J/goC

Your answer should follow the format:

a) q of the water

b) mols of unknown materials

c) ΔHcomb of unknown material with units (2 marks)

2h2o2--> 2h2o + o2

this reaction is of the spontaneous decomposition of hydrogen peroxide down into water and oxygen.

add 2 molecules of hydrogen peroxide and 2 molecules of water. since oxygen is naturally diatomic, the total number of atoms of each element is now the same on both sides of the equation so it is balanced.

this may not be entirely correct but let me know.

the atomic number will stay the same no matter how many electrons it has, so it doesn’t decrease nor increase. it’ll only change with a different number of protons