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
irina1246 [14]
2 years ago
15

How many molecules of O₂ will be required to produce 28.8 g of water? 2H₂ + O₂ ---> 2H₂O

Chemistry
1 answer:
juin [17]2 years ago
4 0

To produce 28.8 g of water 4.81 x 10²³ molecules of O₂ will be required

<h3>What is limiting reagent ?</h3>

The limiting reactant (or limiting reagent) is the reactant that gets consumed first in a chemical reaction and therefore limits how much product can be formed.

According to given equation;

2H₂ + O₂ ---> 2H₂O

If 36 g of H₂O (2 mole) is produced by 1 mole O₂ i.e, 32 gram.

Therefore, 28.8 g of H₂O is produced by ;

32/36 x 28.8 = 25.6 g of O₂

Number of molecules of O₂ = given weight / molecular weight x 6.023 x 10²³

                                              = 25.6 / 32 x 6.023 x 10²³

                                              = 4.81 x 10²³ molecules of O₂

Therefore,4.81 x 10²³ molecules of O₂ will be required to produce 28.8 g of water.

Learn more about Limiting reagent here ;

brainly.com/question/20070272

#SPJ1

You might be interested in
Consider the following reaction between calcium oxide and carbon dioxide: CaO(s)+CO2(g)→CaCO3(s) A chemist allows 14.4 g of CaO
sweet-ann [11.9K]

Answer:

Theoretical yield =26.03 g

Percent yield = 87%

Limiting reactant = CaO

Explanation:

Given data:

Mass of CaO = 14.4 g

Mass of CO₂ = 13.8 g

Actual yield of CaCO₃ = 22.6 g

Theoretical yield = ?

Percent yield = ?

Limiting reactant = ?

Solution:

Chemical equation:

CaO + CO₂   → CaCO₃

Number of moles of CaO:

Number of moles  = Mass /molar mass

Number of moles = 14.4 g / 56.1 g/mol

Number of moles  = 0.26 mol

Number of moles of CO₂:

Number of moles = Mass /molar mass

Number of moles = 13.8 g / 44 g/mol

Number of moles = 0.31 mol

Now we will compare the moles of CO₂ and CaO with CaCO₃ .

                  CO₂         :                CaCO₃  

                  1               :                 1

                 0.31           :              0.31

                CaO           :               CaCO₃  

                 1                :                 1

                 0.26         :              0.26

The number of moles of  CaCO₃ produced by CaO are less it will be limiting reactant.

Mass of CaCO₃: Theoretical yield

Mass of CaCO₃ = moles × molar mass

Mass of CaCO₃ =0.26 mol × 100.1 g/mol

Mass of CaCO₃ =  26.03 g

Percent yield:

Percent yield = actual yield / theoretical yield × 100

Percent yield = 22.6 g/ 26.03 g × 100

Percent yield = 0.87× 100

Percent yield = 87%

Limiting reactant:

The number of moles of  CaCO₃ produced by CaO are less it will be limiting reactant.

7 0
3 years ago
Which is NOT a way that Carbon is released in to the atmosphere?
amid [387]

Answer:

hi, how are you ?

Explanation:

8 0
2 years ago
Read 2 more answers
In the Haber reaction, patented by German chemist Fritz Haber in 1908, dinitrogen gas combines with dihydrogen gas to produce ga
Reptile [31]

Answer:

The rate at which ammonia is being produced is 0.41 kg/sec.

Explanation:

N_2+3H_2\rightarrow 2NH_3 Haber reaction

Volume of dinitrogen consumed in a second = 505 L

Temperature at which reaction is carried out,T= 172°C = 445.15 K

Pressure at which reaction is carried out, P = 0.88 atm

Let the moles of dinitrogen be n.

Using an Ideal gas equation:

PV=nRT

n=\frac{PV}{RT}=\frac{0.88 atm\times 505 L}{0.0821 atm l/mol K\times 445.15 K}=12.1597 mol

According to reaction , 1 mol of ditnitrogen gas produces 2 moles of ammonia.

Then 12.1597 mol of dinitrogen will produce :

\frac{2}{1}\times 12.1597 mol=24.3194 mol of ammonia

Mass of 24.3194 moles of ammonia =24.3194 mol × 17 g/mol

=413.43 g=0.41343 kg ≈ 0.41 kg

505 L of dinitrogen are consumed in 1 second to produce 0.41 kg of ammonia in 1 second. So the rate at which ammonia is being produced is 0.41 kg/sec.

6 0
3 years ago
Need structural formula for each 12, HOCH a CH 1 Dipherylamine.
guajiro [1.7K]
12) Ethylene glycol and <span>Diphenylamine
</span>
<span>attached images
</span>
hope this helps!

5 0
3 years ago
 A chemist describes a particular experiment in this way: "0.0400 mol of H2O2 decomposed into 0.0400 mol of H2O and 0.0200 mol o
AleksandrR [38]
Description:

<span>"0.0400 mol of H2O2 decomposed into 0.0400 mol of H2O and 0.0200 mol of O2." 

This means that a certain amount of H2O2 (0.0400 mol) decomposed or was broken down into two components, 0.04 mol of H2O and 0.02 mol of O2. To examine the system, we need a balanced equation:

H2O2 ---> H2O + 0.5O2

The final concentrations of the system indicates that the system is in equilibrium. </span>
4 0
3 years ago
Other questions:
  • An element is a pure substance that is defined by the number of protons in which is defined as the atomic number
    11·1 answer
  • Which equivalent factor should you use to convert from 4.28 * 10^19 molecules of oxygen to moles of O2
    13·1 answer
  • A shopping cart is a compound machine that makes doing work easier. Compound
    15·1 answer
  • Which of the below options is not a type of chemical bond?
    13·1 answer
  • What are the three types of symbiotic relationships?
    5·2 answers
  • Explain why vanadium (radius=134 pm) and copper (radius=128 pm) have nearly identical atomic radii, even though the atomic numbe
    12·1 answer
  • The shape of the illuminated portion of the Moon as seen by an observer, usually on Earth:
    13·1 answer
  • A student is studying the boiling points of six different liquids and finds results with consistently higher boiling points than
    15·1 answer
  • Use the Bohr Model below to answer the questions:
    6·1 answer
  • Calculate the de broglie wavelength of a subatomic particle that is moving at 351 km/s if its mass is 9.11 à 10â31 kg. λ = hmuh
    12·1 answer
Add answer
Login
Not registered? Fast signup
Signup
Login Signup
Ask question!