Methane combusts according to the following thermochemical equation: CH4(g) + 2O2(g) → CO2(g) + 2H2O(l) ΔH = -891 kJ

If 25 g of methane combusts, how much energy is released in the reaction?
(Show all work and answer with the correct significant figures and units.)

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Explanation:

"among the transition metal elements, manganese and zinc have a slight lowering of electronegativities. the reason behind this is that the nuclear charges of these elements are slightly weaker than the other transition metal elements due to the way their valence electrons are filled up. both manganese and zinc have their valence electrons filled up to the 4th shell with 1 pair of electrons (4s2) completely occupying it. although the electrons in the 3rd shell (3d) are yet to be paired since the outer most shell is filled up, the ability of the nucleus to attract electrons is lessened. hence,   the electronegativity (or the ability to attract electrons) is lessened."

your answer is a. the enthalpy of formation for a pure element in its standard state is always positive.