1answer.
Ask question
Login Signup
Ask question
All categories
  • English
  • Mathematics
  • Social Studies
  • Business
  • History
  • Health
  • Geography
  • Biology
  • Physics
  • Chemistry
  • Computers and Technology
  • Arts
  • World Languages
  • Spanish
  • French
  • German
  • Advanced Placement (AP)
  • SAT
  • Medicine
  • Law
  • Engineering
k0ka [10]
4 years ago
5

* Need ASAP * Explain the relationship between percent composition, Empirical formula, and molecular formula.

Chemistry
1 answer:
sweet-ann [11.9K]4 years ago
5 0

By dividing the percentage composition with the molar mass of that element we will get the empirical formula. Then using that empirical formula and formula mass we can find the molecular formula.

<u>Explanation:</u>

The chemical properties of any substance are defined obviously by the different types and relative amounts of atoms constituting its primary entities (in case of covalent compounds the primary entities are molecules and ions in the event of ionic compounds).

A percent composition of any compound gives the mass percent of each element present in the compound; in addition to that frequently it is determined experimentally and utilized to derive an empirical formula of any compound. An empirical formula mass of any covalent compound could be comparable with the molar or molecular mass of a compound to acquire a molecular formula.

You might be interested in
To the nearest 0.5 mL, what is<br> the water volume in the<br> graduated cylinder?<br> mL?
AnnZ [28]

Answer:

14cm^3

Explanation:

6 0
3 years ago
2C2H2 + 5O2 → 4CO2 + 2 H2O How many grams of CO2 are required to react with exactly 3.00 mol of O2? 106 g 132 g 165 g 76.8 g
cricket20 [7]

Hey there!:

Given the reaction:

2 C2H2 + 5 O2 → 4 CO2 + 2 H2O

5 moles O2 ------------- 4 moles CO2

3.00 moles O2 ----------  ( moles of CO2 ?? )

moles of CO2 = 3.00 * 4 / 5

moles of CO2 =  12 / 5

moles of CO2 = 2.4 moles

So, molar  mass CO2 = 44.01 g/mol

Therefore:

1 mole CO2 -------------- 44.01 g

2.4 moles CO2 ---------- ( mass of CO2 )

mass of CO2 = 2.4 * 44.01 / 1

mass of CO2 = 106 g

Answer A


Hope that helps!

8 0
4 years ago
Which of the following is an example of an action done to maintain homeostasis?
Naddika [18.5K]
Ribosomes hope this helps if not oh well
6 0
3 years ago
A mixture of 10.0 g of Ne and 10.0 g Ar have a total pressure of 1.6 atm. What is the partial pressure of Ne?
Natasha2012 [34]
If u add u will get ur answer
7 0
4 years ago
Read 2 more answers
In a 71.4 g sample of nahco 3 3 ​ , how many grams of sodium are present?
sweet [91]

There are 19.5 g Na in 71.4 g NaHCO₃

Calculate the <em>molecular mass of NaHCO₃</em>.

1 Na = 1 × 22.99 u = 22.99   u

1 H   = 1 × 1.008 u =    1.008 u

1 C   = 1 × 12.01  u =  12.01    u

3 O = 3 × 16.00 u =  <u>48.00  u </u>

               TOTAL =  84.008 u

So, there are 22.99 g of Na in 84.008 g NaHCO₃.

∴ Mass of Na = 71.4 g NaHCO₃ × (22.99 g Na/84.008 g NaHCO₃) = 19.5 g Na

4 0
3 years ago
Other questions:
  • A chemist dissolves 239 mg of pure potassium hydroxide in enough water to make up of solution. Calculate the pH of the solution.
    11·1 answer
  • What is the wavelength in picometers for an electron with 360 eV of kinetic energy?
    10·1 answer
  • Why is electron capture accompanied by the emission of an X-ray?
    6·1 answer
  • No pain no gain . which figure of speech is this​
    12·2 answers
  • I need help asap please help me
    5·2 answers
  • Which products would form if chlorine gas was bubbled through a solution of sodium bromide?
    10·2 answers
  • 3. Describe como se comparan las fuerzas intermoleculares.
    13·1 answer
  • Pb(NO3)2 (aq) + 2 NaI (aq) --&gt; PbI2 (s) + 2 NaNO3 (aq)
    12·1 answer
  • If I have 22,9 moles of a gas at a pressure of 12.4 atm and a volume of 24 liters, what is the temperature?
    12·1 answer
  • Express your answer as a complete ionic equation including phases. Enter a balanced complete ionic equation for
    5·1 answer
Add answer
Login
Not registered? Fast signup
Signup
Login Signup
Ask question!