Which of the following correctly illustrates the mass of reactants and products for the reaction below?

4na + o2 --> 2na2o

92 g na, 32 g o2, 108 g na2o

23 g na, 16 g o2, 124 g na2o

92 g na, 16 g o2, 124 g na2o

23.0 g na, 16 g o2, 39 g na2o

The mass of reactants and products for the reaction is this:

- 92 g Na, 32 g O₂, 124 g Na₂O

which is not a choice from the list.

Explanation:

4 moles of Na reacts with 1 mol of oxygen to produce 2 moles of sodium oxide.

Na = 23 g/m

4 moles are (4 . 23) = 92 g

O₂ = 32 g/m

It's a diatomic molecule (each O is 16 g/m)

Na₂O = 62 g/m

2 mol of sodium oxide will be (2 .62) = 124 grams

The mass of reactants and products for the reaction is this:

- 92 g Na, 32 g O₂, 124 g Na₂O

which is not a choice from the list.

the reaction mixture contains some ammonia, plus a lot of unreacted nitrogen and hydrogen. the mixture is cooled and compressed, causing the ammonia gas to condense into a liquid. the liquefied ammonia is separated and removed. the unreacted nitrogen and hydrogen are then recycled back into the reactor .

i would say b

explanation:

but i think i would need more information than that