Question

Given a compound with a mw of 169 amu having 13.60% na, 8.29% n, 35.51% c, 4.77% h, and 37.85% o, determine the number of each atom present in the compounds formula?

Answer 1

1) Percent composition

Na: 13.60%,
N:     8.29%
C:    35.51%
H:      4.77%
O:   37.85%
     -------------
       100.02%

2) Convert mass percent to molar composition

For that, divide the percent of each element by its atomic mass.


Na: 13.60 / 22.99 = 0.5916
N:     8.29 / 14.01 = 0.5917
C:    35.51 / 12.01 = 2.9567
H:      4.77 / 1.01 = 4.7228
O:   37.85 / 16.00 = 2.3656

3) Divide each number by the smallest one:


Na:  0.5916 / 0.5916 = 1.0
N:     0.5917 / 0.5916 = 1.0
C:    2.9567 / 0.5916 = 5.0
H:      4.7228 / 0.5916 = 8.0
O:   2.3656 / 0.5916 = 4.0

4) State the empirical formula: Na N C5 H8 O4

5) Calculate the mass of the empirical formula:

Multiplicate the number of each atoms times the atomic mass corresponding atomic mass of the atom.

1 * 22.99 + 1 * 14.01 + 5 * 12.01 + 8 * 1.01 + 4 * 16.00 = 169.13

6) Divide the molar mass by the mass of the empirical formula:

169 / 169.13 = 1

7) Conclusion: the molecular formula is Na N C5 H8 O4, so the number of atoms present in the compound formula are:

Na: 1
N: 1
C: 5
N: 8
O: 4

Answer 2

The number of atoms making up the compound is

Na = 1, N = 1, C = 5, H = 8 and O = 4

$\boxed{\boxed{\bold{Further~explanation}}}$

The empirical formula is the smallest comparison of atoms of compound forming elements.

A molecular formula is a formula that shows the number of atomic elements that make up a compound.

(empirical formula) n = molecular formula

The principle of determining empirical formula and molecular formula

• Determine the mass ratio of the constituent elements of the compound.

• Determine the mole ratio by dividing the elemental mass with the relative atomic mass obtained by the empirical formula

• Determine molecular formulas by looking for values of n

Percentage of elements A and B in AxBy compounds:

% A in AₓBy = (x x Ar A / Mr AₓBy) x% AₓBy

% B in AₓBy = (y x Ar B / Mr AₓBy) x% AₓBy

It is known about the% mass of each element

To find the empirical formula, we look for its mole ratio (% mass/ its relative atomic mass)

Na = 13.6 / 23 = 0.5913

N = 8.29 / 14 = 0.5921

C = 35.51 / 12 = 2.9592

H = 4.77 / 1 = 4.77

O = 37.85 / 16 = 2.3656

To simplify the comparison as an integer, we divide by the mole ratio of the smallest element

Na = 0.5913 / 0.5913 = 1

N = 0.5921 / 0.5913 = 1

C = 2.9592 / 0.5913 = 5

H = 4.77 / 0.5913 = 8

O = 2,3656 / 0,5913 = 4

So the empirical formula:

NaNC5H8O4

We look for the molecular formula to get the number of atoms making up the compound

(NaNC5H8O4) n = Mr compound

(1.23 + 14.1 + 5.12 + 8.1 + 4.16) n = 169

(169) n = 169

n = 1

So that the empirical formula and molecular formula are the same so that the number of atoms making up the compound is

Na = 1, N = 1, C = 5, H = 8 and O = 4

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Keywords: empirical formula, molecular formula, mass, mole