Question

The simplest formula for a compound made from element x this 21 nitrogen by mass is

Answer 1

The simplest formula for a compound made from element x which is molar mass is equals to 79.0 g/mol that is 21% nitrogen by mass is X sub 2 N sub 3. In addition, X is equals to 79.0 and N is equals to 14. 

Answer 2

The question seems to be incorrect and here is a feel of what the question is all about.

The simplest formula for a compound made from element X (molar mass = 79.0 g/mol) that is a 21.0% nitrogen by mass is:

The objective of this question is for us to determine the chemical compound from the parameters given in the given question.

From the question, the elements are X (unknown) and N (Nitrogen).

Given that,

• the mass percentage of Nitrogen = 21.0%

Then,

• the  remaining mass percentage of the X(unknown) is:

= 100% - 21.0%

= 79.0 %

In a 100 g of the compound, their respective mass will be as follows:

For X:

= 21.0% × 100.0 g

= 0.21 × 100.0 g

= 21.0 g

For N:

= 79.0% × 100.0 g

= 0.79 × 100.0 g

= 79.0 g

Since their mass is known, we can calculate their respective number of moles.

Using the relation:

$\mathbf{number \ of \ moles = \dfrac{mass}{molar \ mass}}$

number of moles of 79.0 g of X is:

$\mathbf{\dfrac{79.0 \ g \ X }{79.0 \ g/mole \ X}}$

= 1.00 mol of X

number of moles of 21.0 g of N is

recall that:

the molar mass of N = 14

$= \mathbf{\dfrac{21.0 \ g \ N }{14.0 \ g/mole \N}}$

= 1.50 mol of N

Using the empirical formula method, we divide each number of moles by the smallest mole.

∴

For X, we have:

$\mathbf{\dfrac{1.00 \ mol \ of \ X }{1.00 \ mol } = 1.00 \ X}$

For N, we have;

$\mathbf{\dfrac{1.50 \ mol \ of \ N }{1.00 \ mol } = 1.50 \ N}$

The ratio of N to X is 1.50N: 1.00X

Let's multiply both values by two(2) to have a whole number.

By doing so, we have:

= 3N: 2X

= X₂N₃

Therefore, we can conclude that the simplest formula for the compound is:

X₂N₃

Learn more about empirical formula here:

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