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3 years ago

What is the percentage sodium in sodium oxide

Chemistry

2 answers:

Sav [38]3 years ago

5 0

Sodium oxide =-N220 i think

Alekssandra [29.7K]3 years ago

4 0

<span>
Sodium Oxide= Na2O
The formula mass of Na2O is (2x23) + 16 = 62g/mol

% Na= (46/62) x 100 = 74%
% O= (16/62) x 100 = 26%</span><span>
</span>

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How many atoms are found in 4.75 moles of Fe?

aliya0001 [1]

Answer:

The answer to your question is below

Explanation:

Number of atoms = ?

moles of Fe = 4.75

-Use proportions to solve this problem

1 mol of Fe --------------------- 6.023 x 10²³ atoms

4.75 moles --------------------- x

x = (4.75 x 6.023 x 10²³) / 1

x = 2.86 x 10²⁴ / 1

Number of atoms = 2.86 x 10²⁴

Number of moles = ?

moles of 1.058 moles of H₂O

I think this question is incorrect, maybe you wish to know the number of atoms or grams of H₂O.

Number of atoms = ?

moles of Fe = 0.759

1 mol of Fe ------------------ 6.023 x 10²³ atoms

0.759 moles --------------- x

x = (0.759 x 6.023 x 10²³) / 1

x = 4.57 x 10²³ / 1

Number of atoms of Fe = 4.57 x 10²³ atoms

Number of molecules = ?

moles of H₂O = 3.5 moles

1 mol of H₂O ------------------ 6.023 x 10²³ molecules

3.5 moles ------------------ x

x = (3.5 x 6.023 x 10²³) / 1

x = 2.11 x 10²⁴ molecules

Number of molecules = 2.11 x 10²⁴

7 0

3 years ago

Which of the following chemical equations proves that the law of conservation of mass is in effect?

bogdanovich [222]

Answer:

2KCl + F₂ → 2KF + Cl₂

Explanation:

Law of conservation of mass:

According to the law of conservation mass, mass can neither be created nor destroyed in a chemical equation.

This law was given by French chemist Antoine Lavoisier in 1789. According to this law mass of reactant and mass of product must be equal, because masses are not created or destroyed in a chemical reaction.

2KCl + F₂ → 2KF + Cl₂

In this equation mass of reactant and product is equal. There are 2 potassium 2 chlorine and fluorine atoms on both side of equation it means mass remain conserved.

All other options are incorrect because mass is not conserved.

Mg₂ + LiBr ---> LiMg + Br

In this equation mass of magnesium is more on reactant side.

Na +O₂ ---> Na₂O

In this equation there is more oxygen and less sodium on reactant side while there is more sodium and less oxygen on product side.

H₂O ---> H₂ + O₂

In this equation there is less oxygen on reactant side while more oxygen on product side.

5 0

3 years ago

Unlike an acid, an aqueous solution of a base

HACTEHA [7]

Answer:

D) contains more OH– ions than H+ ions

Explanation:

THESE ARE THE OPTIONS FOR THE QUESTION

A) causes some indicators to change color B) conducts electricity C) contains more H+ ions than OH– ions D) contains more OH– ions than H+ ions

Base can be regarded as substance which can dissociates in water then form hydroxide ions (OH–) .

Bases can be regarded as compounds which break into hydroxide ions I.e (OH-) with more other compounds if put in an aqueous solution. Hence it contains more OH– ions

3 0

3 years ago

Which of the followin separation methods is used in making coffee at home ?

andre [41]

Yes u are right :) FILTRATION IS THE CORRECT ANSWERR

7 0

3 years ago

Read 2 more answers

Name each of the following molecular binary compounds:

Tanya [424]

Answer:

Explanation:

From the given information; we are to assign the correct naming for the molecular binary compounds.

01. CaCl2 → Calcium CHloride

02. HI (g) → Hydrogen mono iodide gas

03. HI (aq) → Hydroiodic acid

04. BH3 → Borontrihydride

05. Cl2O6 → Dichlorine hexoxide

06. ClF → Chlorine monoflouride

07. P2Cl4 → Phosphorus tetrachloride

08. I2O5 → Diiodine pentaoxide

09. BrF5 → Bromine pentaflouride

10. HBr(aq) → Hydrobromic acid

11. IF7 → Iodine heptaflouride

12. NF3 → nitrogen triflouride

13. H2Se(aq) → hydroselenic acid

14. BrCl → Bromine monochloride

15. H2Se(g) → Hydrogen Selenide

16. SnO2 → Tindeoxide

17. HBr(g) → Hydrogenbromide gas

18. AsF3 → Arsenic triflouride

19. N2O3 → Dinitrogentrioxide

20. IF4 → Iodine pentafluoride

01. hydroiodic acid → HI (aq)

02. hydrogen monoiodide gas → HI (g)

03. diiodine tetraoxide → I2O4

04. bromine monofluoride → BrF

05. silicon tetrahydride → SiH4

06. tetraphosphorus hexaoxide → P4O6

07. disulfur monoxide → S2O

08. carbon monooxide → CO

09. hydrogen monochloride gas → Hcl

10. tetraphosphorus decaoxide → P4O10

11. dibromine monoxide → Br2O

12. dinitrogen tetrafluoride → N2F4

13. disilicon hexahydride → SiH6

14. tetraarsenic hexaoxide → As4O6

15. hydrochloric acid → HCl (aq)

16. arsenic trihydride → AsH3

17. iodine heptafluoride → IF7

18. bromine dioxide → BrO2

19. disulfur decafluoride → S2F10

20. dichlorine heptaoxide → Cl2O7

4 0

3 years ago