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.)
CH4(g) + 202(g) --> CO2(g) + 2H2O(g)deltaH = -891 kJ/mol.
Multipliedby2: = - 1780.8.4k) multipled by ZAH=-
I= -445.2kJ
AH°rxn = [2AHºf(CO2) + 3AHºf(H20)]-[AH°f(C2H5OH) + 3AH° S(02)] = [2( - 393.5kJ).+31 - 2
41.8)] - [ - 277.7) + 3(0)]= -1234.7kJ

yes it is balanced

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explanation:

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in 1783 cavendish was working with his hydrogen gas and found that when he burned it and condensed the vapor it was water. this was very significant since it disproved the greek theory of elements completely since water was not a simple substance but the product of two gases. it was lavoisier who hearing of the experiment gave cavendish's gas the name hydrogen ("water-producer") and added that hydrogen burned by combining with oxygen and that water was a hydrogen-oxygen combination.

explanation:

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