Chemistry, 01.07.2019 21:10 izzy123abc

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?

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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 from: dontcareanyonemo

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

$\boxed{\boxed{\bold{Learn~more}}}$

the molar mass of a substance

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Determine the empirical and molecular formulas

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Determine the molecular formula of the compound

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Keywords: empirical formula, molecular formula, mass, mole

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, de

Answer from: Quest

the correct answer is b. a strong acid completely dissociates to its ions when dissolved in water. $hbr$ completely dissociates to $h^+$ and $br-$ ions. a is incorrect because $h_2s$ does not fully ionize to $h^+$ and $hs^-$ ions and some remain as the compound $h_2s$ . c and d are incorrect because, $li_2o$ and $libr$ do not fall into the category of bronsted lowry acids. a bronsted lowry acid is a proton donor and since both molecules do not have a proton to donate they are not bronsted lowry acids. likewise, if we use the lewis acid definition, they cannot be acids. a lewis acid is an electron pair acceptor. both $li_2o$ and $libr$ have a complete octet so can not accept any electrons which disqualifies them as acids.