Methane combusts according to the following thermochemical equation: CH4 (g) +2O2 (g) - CO2 (g) + 2H2O(I) AH = -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:

the ideal gas law equation is as follows

pv = nrt

where p - pressure

v - volume

n - number of moles

r - universal gas constant

t - temperature

so if the pressure, volume and temperature are already known

we are left with n and r

since r is the universal gas constant that has a known fixed value then r too is known

so we are left with 'n'

once we know temperature volume and pressure

we can find the number of moles of gas present using the ideal gas law equation

this is not my own answer, this is an answer for the same question by the user blahblahmali. i do not claim ownership of this account.

c. orbital shape i hope this is correct