I also need help with this please
The gas-phase reaction between ammonia and oxygen occurs only at high temperature. It is referred to as “burning” ammonia, even though no carbon is present.
a. Balance the chemical equation and give states of matter
__NH3( ) + __O2( ) = __NO( ) + __ H2O ( )
b. The reaction is carried out in a sealed flask initially containing 88.5 grams of ammonia and 88.5 grams of oxygen. Which reactant is limiting?
c. What is the maximum number of moles of water that can be formed?
a. 4NH3(g ) + 5O2(g ) = 4NO(g ) + 6H2O (g)
Note: Can't be sure of the physical state of H2O. In a sealed container I assume the temperature will be high enough for H2O to be steam (gas) but as it cools it will be liquid (l).
b. mols NH3 = grams/molar mass = 88.5/17 = 5.2
mola O2 = 88.5/32 = 2.76
H2O formed with 5.2 mols NH3 and excess O2 = 5.2 x (6 mols H2O/4 mols NH3) = 5.2 x 6/4 = 7.8 mols H2O
H2O formed with 2.76 mols O2 and excess NH3 = 2.76 x 6(6 mols H2O/5 mols H2O) = 3.32
In limiting reagent problems the smaller number always wins because you can't get more than the smallest amount so O2 is the limiting reagent.
c. See answer to b.