Answer:
D. N₂O
Explanation:
Let's assume we have 100 g of the compound. That means it consists of 63.61 grams of nitrogen and 36.69 grams of oxygen.
Converting masses to moles:
63.61 g N × (1 mol N / 14.01 g N) = 4.540 mol N
36.69 g O × (1 mol O / 16.00 g O) = 2.293 mol O
Normalize by dividing by the smallest:
4.540 / 2.293 = 1.980 mol N
2.293 / 2.293 = 1.000 mol O
So there is approximately twice as many N atoms as O atoms. The empirical formula is therefore N₂O.
The heat that is needed to raise the temperature of 78.4 g of aluminium from 19.4 °c to 98.6°c is 5600.77 j
<u><em>calculation</em></u>
Heat(Q) = mass(M) x specific heat capacity (C) x change in temperature(ΔT)
where;
Q=?
M = 78. 4 g
C=0.902 j/g/c
ΔT=98.6°c -19.4°c =79.2°c
Q is therefore = 78.4 g x 0.902 j/g/c x 79.2°c =5600.77 j
Generally speaking a precipitate is something that will form as a result of the reaction. It generally is a solid material.
Sodium and nitrates are soluble so Calcium Phosphate would precipitate out....
