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astra-53 [7]
3 years ago
15

Which is a product in the following chemical reaction? CH4 + 2O2 → CO2 + 2H2O

Chemistry
2 answers:
NeX [460]3 years ago
5 0
<span>CH4 + 2O2 → CO2 + 2H2O
</span>
The products are water (H2O) and carbon dioxide (CO2)
Kobotan [32]3 years ago
5 0

Answer : The product in the given chemical reaction are, carbon dioxide (CO_2) and water (H_2O).

Explanation :

The given balanced chemical reaction is,

CH_4+2O_2\rightarrow CO_2+2H_2O

The give balanced chemical reaction is a balanced reaction because in this reaction all the atoms of individual elements are completely balanced.

In the chemical reaction, the species present on left side of the right arrow are the reactants and species present on right side of the right arrow are the products.

CH_4 and O_2 are the reactants.

CO_2 and H_2O are the products.

Hence, the product in the given chemical reaction are, carbon dioxide (CO_2) and water (H_2O).

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Answer:

14.0067 g/mol

Explanation:

The molar mass of pure nitrogen is 14.0067 because when you look at the top right of an element on the periodic table of elements you can see the molar mass of an element. This can go for any other elements on the table, just look at the top right of the box. The molar mass of an element is also called the atomic weight. Hope this helps! :)

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Find the equilibrium value of [CO] if Kc=14.5 : CO (g) + 2H2 (g) ↔ CH3OH (g) Equilibrium concentrations: [H2] = 0.322 M and [CH3
Annette [7]

Answer:

The equilibrium value of [CO] is 1.04 M

Explanation:

Chemical equilibrium is the state to which a spontaneously evolving  chemical system, in which a reversible chemical reaction takes place.  When this situation is reached, it is observed that the  concentrations of substances, both reagents and reaction products,  they remain constant over time. That is, the rate of reaction of reagents to products is the same as that of products to reagents.

Reagent concentrations  and products in equilibrium are related by the equilibrium constant Kc. Being:

aA + bB ⇔ cC + dD

Kc=\frac{[C]^{c} *[D]^{d} }{[A]^{a} *[B]^{b} }

Then this constant Kces equals the multiplication of the concentrations of the products raised to their stoichiometric coefficients between the multiplication of the concentrations of the reactants also raised to their stoichiometric coefficients.

In this case:

Kc=\frac{[CH_{3}OH ]}{[CO]*[H_{2} ]^{2} }

You know:

  • Kc= 14.5
  • [H₂]= 0.322 M
  • [CH₃OH] =1.56 M

Replacing:

14.5=\frac{1.56}{[CO]*0.322^{2} }

Solving:

[CO]=\frac{1.56}{14.5*0.322^{2} }

[CO]= 1.04 M

The equilibrium value of [CO] is 1.04 M

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Answer:

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