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Savatey [412]
3 years ago
11

you find that 7.36g of a compound has decomposed to give 6.93g of oxygen. the only other element in the compound is hydrogen. if

the molar mass of the compound is 34.0g/mol, what is its molecular formula?
Chemistry
2 answers:
slavikrds [6]3 years ago
8 0
First solve the moles of oxgen present in the compound

mol O = 6.93 g O ( 1 mol O / 16 g O )
mol O = 0.43 mol H

then solve the moles of hydrogen present
mol H = ( 7.36 - 6.93) g H ( 1 mol H / 1 g H)
mol H = 0.43 mol H
so the O and H are in the same mole content so the molecular formula would be OH, but the molar mass will not satisfy. so the answer would be
H2O2

natta225 [31]3 years ago
6 0

Answer:

H2O2.

Explanation:

Okay, from the question we can see that the compound contains only two elements, that is, Hydrogen and Oxygen. Also,in the question we have some parameters, they are;

Mass of the Compound = 7.36 grams.

The compound decomposed to give Oxygen, the mass of the oxygen is equal to 6.93 grams.

The first thing to do is to determine the number of moles. The number of moles will now be used to determine the molecular formula of the compound.

To calculate the number of moles,n we need the formula below:

Number of moles,n= mass(in grams)/molar mass (In grams per mol). -----------------------------------------(1).

===> Numbers of moles,n= 6.93 grams ÷ 16 grams per mole.

==> 0.433125 mol of oxygen

So, the total mass of the compound= mass of Hydrogen + mass of Oxygen. -----------------------------------------------------(2).

7.36 grams = mass of Hydrogen + 6.93 grams.

==> Mass of Hydrogen = 7.36 grams - 6.93 grams = 0.43 grams.

Using equation (1), the number of moles of Hydrogen: Molar mass of

===>0.43/ 1.00784 grams per mol.

= 0.43 mol.

Hence, there is a need for us to divide both moles by the smaller but since we both are the same, we will just pick on. Therefore, for oxygen and hydrogen it is going to be 1:1.

So, (16+1) b = 34 g/mol

===> 34/17=b= 2.

Hence, 2{OH} = H2O.

The decomposition Reaction is given below;

2 H2O2 --------> 2 H2O + O2

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Chemical element that has atomic number less than 58 and atomic mass greater than 135.6
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A chemical element that has an atomic number less than 58 and an atomic mass greater than 135.6m is barium (atomic no. 56 and atomic mass137.13 ) and lanthanum (atomic no. 57  and atomic mass 135.6).

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Barium is an element with the symbol Ba and atomic number 56. It is an alkaline earth metal that is soft and silvery, and it is the fifth element in group 2. Barium is never found in nature as a free element due to its extreme chemical reactivity. Oil well drilling fluid uses barium sulfate as an insoluble ingredient. It is employed as an X-ray radiocontrast agent in a purer form to image the human gastrointestinal tract. Barium compounds that dissolve in water have been employed as rodenticides despite being hazardous.

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Chemical element lanthanum has the atomic number 57 and the symbol La. It is a silvery-white, ductile, soft metal that slowly tarnishes when exposed to air. It serves as the eponym for the group of 15 related elements in the periodic table between lanthanum and lutetium, of which lanthanum is the first and prototype. The rare earth elements traditionally include lanthanum.

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Two types of heterogeneous mixtures are suspensions and colloids.<br>true or false<br><br>​
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The properties of the mixture like concentration may change for different parts of the mixture.

Colloids contain solute particles of size 2nm-500nm.The presence of these particles makes the mixture heterogeneous.

Suspensions contain solute particles of size 500nm-1000nm.These particles settle to the bottom of the mixture which makes the composition of the bottom different from the top.

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It is given that,

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The radius of the orbit in which time period is 8T is R'. So, the relation is given by :

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