2nh3 + 2 o2 → n2o + 3 h2o if 80.0 grams of o2 are reacted in the above reaction, how many grams of n2o will be produced (mm o2=32 g/mol; nh3=17.04 g. mol, n2o=44.02 g/mol, h2o=18.02 g/mol)? 29.1 g 67.6 g 55.0 g 165 g

   2 NH3 + 2 O2 → N2O + 3 H2O

mass of O2 = 80.0g

moles of O2 = 80.0/32 = 2.5 moles O2

moles of N2O = 2.5 moles O2 x   1 mole N2O      = 1.25 moles N2O

                                                       2 moles of O2

mass of N2O produced ;

moles = mass/Molar mass

mass = moles x Molar mass

        = 1.25 x 44.02

        = 55.025 g N2O

55.025g of N2O is produced in this reaction.

the electronic configuration of an atom with eight electrons is 1s²2s²2p⁴. the orbital diagrams are shown in the figure.

as per the hunds rule:

1. electrons tend to avoid being in the same orbital as per as practicable.

2. electrons in different orbitals of the same energy will have their spin parallel.

this can be illustrated from the multiplicity of the orbitals of the atom. as there are four electrons in the p orbital and p orbital has 3 sub-shells. the electrons can be fed in different ways as shown in the figure but the correct orbital diagram will be as per the hunds rule.

2b2t

explanation:

2b2t