What observations support the assumption that all of the iodine reacted with the zinc explain?
1 answer:
Answer: It will lead to form a white colored product .
Explanation: The reaction of iodine and zinc involves the direct reaction between a metal and a non-metal leading to the synthesis of a metal salt.
During this reaction, heat is released (exothermic reaction) while forming Zinc Iodide() which can be easily obtained by evaporating the solvent.
By looking at the stoichiometric coefficients of reactants and products, we observe that whole of the iodine has reacted with zinc.
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Answer: 1. The empirical formula is
2. The molecular formula is
Explanation:
If percentage are given then we are taking total mass is 100 grams.
So, the mass of each element is equal to the percentage given.
Mass of P = 37.32 g
Mass of N = 16.88 g
Mass of F = 45.79 g
Step 1 : convert given masses into moles.
Moles of P =
Moles of N =
Moles of F =
Step 2 : For the mole ratio, divide each value of moles by the smallest number of moles calculated.
For P =
For N =
For F =
The ratio of P: N: F= 1: 1: 2
Hence the empirical formula is
The empirical weight of = 1(31)+1(14)+2(19)= 82.98 g.
The molecular weight = 82.98 g/mole
Now we have to calculate the molecular formula.
The molecular formula will be=