To identify a diatomic gas (x2), a researcher carried out the following experiment: she weighed an empty 5.8-l bulb, then filled it with the gas at 1.00 atm and 21.0 ∘c and weighed it again. the difference in mass was 6.7 g. identify the gas. express your answer as a chemical formula.

Explanation:

The given data is as follows.

      Volume = 5.8 L,    Pressure = 1.00 atm

      T = = (21 + 273) K = 294 K,   mass = 6.7 g

     R = 0.0821 Latm/mol K

According to the ideal gas equation, we will calculate the number of moles as follows.

             PV = nRT

or,          n =

Hence, putting the given values into the above formula as follows.

               n =

                  =

                  = 0.24 mol

Now, calculate molar mass of the gas as follows.

            Molar mass =

                                =

                                = 27.91 g/mol

or,                             = 28 g/mol (approx)

As the gas is diatomic so, mass of two atoms of gas X is 28 g/mol. And, mass of one atom of gas is as follows.

                          = 14 g/mol

Hence, nitrogen atom has a mass of 14 g/mol. Therefore, we can conclude that the given diatomic gas is .

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.  

the correct answer is option d

explanation:

i was wrong its d because they dont use cm when calculating square roots