The specific heat capacity of liquid water is 4.186 J/gm K. This means that each gram of liquid water requires 4.186 Joules of heat energy to raise its temperature by one degree Kelvin. One molar mass of water is equivalent to 18 grams. Therefore, the molar heat capacity becomes the product of 4.186 and 18
Answer:
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Explanation:
1. Thermochemical equation is balance stoichiometric chemical equation written with the phases of the reactants and products in the brackets along with the enthalpy change of the reaction.
The given correct thermochemical reactions are:
![Fe(s)+O_2(g)\rightarrow Fe_2O_3(s),\Delta H = 3,926 kJ ](https://tex.z-dn.net/?f=Fe%28s%29%2BO_2%28g%29%5Crightarrow%20Fe_2O_3%28s%29%2C%5CDelta%20H%20%3D%203%2C926%20kJ%0A)
![C_3H_8(g)+5O_2 (g)\rightarrow 3CO_2 (g)+4H_2O(l),\Delta H= 2,220 kJ/mol](https://tex.z-dn.net/?f=C_3H_8%28g%29%2B5O_2%20%28g%29%5Crightarrow%203CO_2%20%28g%29%2B4H_2O%28l%29%2C%5CDelta%20H%3D%202%2C220%20kJ%2Fmol)
2. Phase change affect the value of the enthalpy change of the thermochemical equation. This is because change in phase is accompanied by change in energy. For example:
![H_2O(s)\rightarrow H_2O(g),\Delta H_{s}=51.1 kJ/mol](https://tex.z-dn.net/?f=H_2O%28s%29%5Crightarrow%20H_2O%28g%29%2C%5CDelta%20H_%7Bs%7D%3D51.1%20kJ%2Fmol)
![H_2O(l)\rightarrow H_2O(g),\Delta H_{v}=40.65 kJ/mol](https://tex.z-dn.net/?f=H_2O%28l%29%5Crightarrow%20H_2O%28g%29%2C%5CDelta%20H_%7Bv%7D%3D40.65%20kJ%2Fmol)
In both reaction phase of water is changing with change in energy of enthalpy of reaction.
PH is the potential of hydrogen, pH provides a measure of the concentration of hydrogen ion while pOH scale provides the concentration of OH- ions.
pH denotes the negative logarithm of concentration of hydrogen while pOH denotes the negative logarithm of the concentration OH- ions.
Therefore; in this case the pOH= -log (OH-)
= - log (10^-10)
= 10
If the pOH is 10 then the pH of the solution will be 4