For the chemical reaction below, determine the amount of HI produced when 3.32E+0 g of hydrogen is reacted with 5.064E+1 g of iodine to produce hydrogen iodide (HI). H(g) + I(g) → 2HI(g)

 The amount of HI produced is 102 g

Explanation:

To calculate the number of moles, we use the equation:

     .....(1)

For hydrogen:

Given mass of hydrogen =

Molar mass of hydrogen= 2 g/mol

For iodine:

Given mass of iodine =  

Molar mass of iodine= 127 g/mol

The chemical equation for the reaction is:

By Stoichiometry of the reaction:

1 mole of iodine reacts with 1 mole of hydrogen

So, 0.399 moles of  iodine will react with = of hydrogen

As, given amount of hydrogen is more than the required amount. So, it is considered as an excess reagent.

Thus, iodine is considered as a limiting reagent because it limits the formation of product.

By Stoichiometry of the reaction:

1 moles of iodine produces 2 mole of hydrogen iodide

So, 0.399 moles of iodine will produce = of hydrogen iodide

The amount of HI produced is 102 g

answer: option (b) is the correct answer.

explanation:

a covalent bond is formed by sharing of electrons. whereas polarity arises due to difference in electronegativity of two atoms.

therefore, more is the electronegativity of an atom which combines with the titanium, more readily it will induce a partial positive and negative charge.

thus, out of the given options fluorine is most electronegative and has an incomplete octet. therefore, it will readily combine with titanium to share the electrons and complete its octet.