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
Ket [755]
3 years ago
7

Consider a reaction in which hydrogen (H2) and oxygen (O2) react to form water (H2O). By mass, the mixture of reactants is 1 par

t hydrogen and 6 parts oxygen. Write the chemical reaction showing reactant and products including any leftover oxygen or hydrogen. Calculate the equivalence ratio for this reaction.
Chemistry
1 answer:
Murrr4er [49]3 years ago
6 0

Answer:

equivalence ratio= 0.08333

Explanation:

The balanced stoichoimetric equation tells us the amount of hydrogen in moles required to react with a specific amount of oxygen in moles to produce water. The Balanced equation of the reaction is shown

2H_{2}+O_{2}  → 2 H_{2}O

this means 2 parts of Hydrogen will react with one part of oxgen to produce 2parts of water as shown above

in the question, 1 part of hydrogen was made to react with 6parts of oxygen. which means comparing with the balanced equation, oxygen is in excess as only \frac{1}{2} part of oxygen will react with 1part of hydrogen. the equation is shown below

1H_{2}+\frac{1}{2} O_{2}  → 1 H_{2}O +\frac{11}{2}O_{2}  

The equivalence ratio is the ratio of actual fuel to air ratio to stoichiometric fuel to air ratio and is calculated as follows:

actual fuel/air ratio = parts of fuel/parts of air

                               =\frac{1}{6}

stoichiometric fuel/air ratio = \frac{2}{1}

equivalence ratio = \frac{actual fuel/air ratio}{stoichiometric fuel/air ratio }

                             =\frac{\frac{1}{6} }{\frac{2}{1} }

                             = 0.08333

Have a great day Jershaun9358

Download docx
You might be interested in
Determine the empirical and molecular formula:
Bingel [31]

Answer:

The empirical formula = molecular formula = C13H18O2

Explanation:

in 100% compound we have 75.6 % Carbon ( Molar mass = 12g/mole), 8.80% hydrogen ( Molar mass = 1.01 g/mole) and 15.5% Oxygen (Molar mass = 16.01 g/mole).

Carbon: 75.6g / 12 = 6.29

Hydrogen: 8.80/ 1 = 8.80

Oxygen: 15.5/ 16 = 0.97

⇒0.97 is the smallest so we divide everything through by 0.97

C: 6.29 / 0.97 =  6.48 ≈ 6.5

H: 8.80 /0.97 = 9

O: 0.97 / 0.97 = 1

To get rid of decimals, we multiply by 2  

C: 6.5 x 2 = 13

H: 9 x 2 = 18

O: 1 x 2 = 2

The empirical formula = C13H18O2

13x 12g/mol + 18x1g/mol  + 2x 16g/mol = 156 + 18 + 32 = 206g/mol  which is the molar mass of ibuprofen

The empirical formula = molecular formula = C13H18O2

6 0
3 years ago
Stained glass consists of colored dyes mixed with silicon dioxide molecules. Variations in the color of the glass occur because
Juli2301 [7.4K]

Answer:

Explanation:

heterogeneous!!!!

6 0
3 years ago
Acetylene gas (ethyne; HC = CH) burns in an oxyacetylene torch to produce carbon dioxide and water vapor. The heat of reaction f
Yanka [14]

The mass of CO2 produced by 26g of acetylene is 88g.

Given ,

In an oxyacetylene torch, acetylene gas (ethyne; HCCH) burns to produce carbon dioxide and water vapour.

The acetylene combustion reaction is given by,

H2O + HCCH + 5/2 O=O 2CO2

Heat of reaction for acetylene combustion = 1259kj/mol

CO2 has a molecular mass of 44g/mol.

2 moles of CO2 have a molecular mass of 88g.

On combustion, 1 mole of acetylene yields 2 moles of CO2.

Thus, 26g of acetylene produces 88g of CO2 when burned.

As a result, the mass of carbon dioxide produced by 26g of acetylene is 88g.

Learn more about acetylene here :

brainly.com/question/15346128

#SPJ4

6 0
1 year ago
How would planting a variety of plants in a vacant (empty) lot help establish an ecosystem in that location?
vichka [17]

the plants would grow  and reproduce working together forming nutrients from their dropped  leaves / branches etc causing insects to come along and do the same  along with animals and a keystone species to form a revolving ecosystem continuing an energy moving process

3 0
3 years ago
What is the empirical formula of C3H6N2
Evgen [1.6K]

Answer:

The empirical formula of the compound C₃H₆N₂ is C₃H₆N₂

Explanation:

The empirical formula of a compound is the formula of the compound given in the (smallest) whole number ratio of the elements of the compound

The empirical formula of S₂O₂ is SO

The empirical formula of C₃H₆O₃ is CH₂O

The given compound's molecular formula is C₃H₆N₂

The smallest whole number ratio of of the elements of the compound is 3:6:2, therefore, the empirical formula of the compound C₃H₆N₂ is C₃H₆N₂.

4 0
3 years ago
Other questions:
  • A solution contains an unknown mass of dissolved barium ions. When sodium sulfate is added to the solution, a white precipitate
    7·1 answer
  • In reversible reaction when do forward reactions take place
    9·1 answer
  • Bases feel slippery because they remove fats and oils from the surface of our skin.
    9·2 answers
  • 2. The formula for density is where m is mass and V is volume. If the volume inside the packet decreases, what would happen to t
    7·1 answer
  • Report the precise concentration of the undiluted stock solution #1 of TZ in micromoles per liter. This is your most concentrate
    7·1 answer
  • Ammonia gas combines with excess oxygen gas to produce nitric oxide and water. How many grams of ammonia gas would have to react
    13·1 answer
  • radiation is the transfer of energy through A: thermal energy B: visible light or C: electromagnetic waves??
    11·1 answer
  • What volume of the 5.00% (w/v) citrie acid solution described above would be needed to provide 738 mg citric acid for a reaction
    10·1 answer
  • Which of the following is NOT an example of proxy data?
    11·1 answer
  • To what pH should you adjust a standard hydrogen electrode to get an electrode potential of -0.128 V ? (Assume that the partial
    9·1 answer
Add answer
Login
Not registered? Fast signup
Signup
Login Signup
Ask question!