Given the following unbalanced thermochemical equation, how much heat will be released from the combustion of 45.5 grams of ch4 in an excess of oxygen gas? ch4(g) + 2o2(g) → co2(g) + 2h2o(l) + 890 kj

CH4 + 2O2 → CO2 + 2H2O + 890 kJ

MM of CH4 = (12.01 + 4x1.008) g/mol = 16.04 g/mol

Moles of CH4 = 45.5 g CH4 x (1 mol CH4/16.04 g CH4) = 2.837 mol CH4

q = 2.837 mol CH4 x (890 kJ/1 mol CH4) = 2520 kJ

-2530kJ

Explanation:

45.5*16*890=2530

"hydrogen bonding is the attraction of h atoms in the water molecule (slight + charge) to o atoms in a neighboring water molecule (slight - charge); it is a weak interatomic force. but it is still strong enough to the water molecules "stick" together."

what does the table look like