Rxn =
Calculate ΔΗο. for the combustion reaction of
CH4 shown below given the following:
AHºf CH4(g) = -74.8 kJ/mol;
AHºf CO2(g) = -393.5 kJ/mol;
AHºf H2O(1) = -285.5 kJ/mol.
CH_(g) + 2 O2(g) > CO2(g) + 2 H2O(1)
=
=
A. -604.2 kJ
B. 889.7 kJ
C. -997.7 kJ
D. -889.7 kJ
E. None of the above

Nitric oxide (no) can be formed from nitrogen, hydrogen and oxygen in two steps. in the first step, nitrogen and hydrogen react to form ammonia: n2(g) + 2 h_2(g) rightarrow 2 nh_3 (g) delta h = -92. kj in the second step, ammonia and oxygen react to form nitric oxide and water: 4 nh_3(g) + 5 o_2(g) rightarrow 4no(g) + 6 h_2o(g) delta h = -905. kj calculate the net change in enthalpy for the formation of one mole of nitric oxide from nitrogen, hydrogen and oxygen from these reactions. round your answer to the nearest .

What causes most sediment to wash or fall into a river

If 3 moles of a compound use 24 j of energy in a reaction, what is the a hreaction in j/mol?