All categories

3 years ago

Consider the following reversible reaction.

Chemistry

2 answers:

Elodia [21]3 years ago

7 0

Answer:

C on edge

Explanation:

got it correct :)

dmitriy555 [2]3 years ago

6 0

Answer:

Keq = [CO₂]/[O₂]

Explanation:

Step 1: Write the balanced equation for the reaction at equilibrium

C(s) + O₂(g) ⇄ CO₂(g)

Step 2: Write the expression for the equilibrium constant (Keq)

The equilibrium constant is equal to the product of the concentrations of the products raised to their stoichiometric coefficients divided by the product of the concentrations of the reactants raised to their stoichiometric coefficients. It only includes gases and aqueous species. The equilibrium constant for the given system is:

Keq = [CO₂]/[O₂]

You might be interested in

Which substance can't be broken down by chemical means?

irina1246 [14]

Antimony cannot be broken down by chemical means because it is an element, a principle building block of matter. All other choices are compounds, which can be separated if put through enough stress to break the bonds between the atoms.

5 0

3 years ago

Given the two half-reactions, what must be done in the next step before the reaction can be balanced? Au3+ --> Au I- --> I

Artyom0805 [142]

Answer:

The balance equation is

$2Au^{+3} + 6I^{-}$ → $2Au + 3I_{2}$

Explanation:

first, we have to make sure that the atoms are balanced

$Au^{+3}$ → $Au^{}$

$2I^{-}$ → $I_{2}$

then we proceed to balance charges of each half-reaction

$Au^{+3} + 3e^{-}$ → $Au^{}$

$2I^{-}$ → $I_{2}$ $+ 2e^{-}$

Now we multiply the half-reactions to match the number of electrons in each one

( $Au^{+3} + 3e^{-}$ → $Au^{}$ )x2

( $2I^{-}$ → $I_{2}$ $+ 2e^{-}$ )x3

and now we do the sum of the half-reactions

2 $Au^{+3} + 6e^{-}$ → 2 $Au^{}$

$6I^{-}$ → 3 $I_{2}$ $+ 6e^{-}$

$2Au^{+3} + 6I^{-}$ → $2Au + 3I_{2}$

note: the only atom that needed to be balanced was I

3 0

4 years ago

Read 2 more answers

What do atoms make up

kumpel [21]

Atoms make upthey make up oxygen

8 0

3 years ago

What is the purpose of galvanization?

frutty [35]

Galvanizing protects from rust in a number of ways: It forms a barrier that prevents corrosive substances from reaching the underlying steel or iron. The zinc serves as a sacrificial anode so that even if the coating is scratched, the exposed steel will still be protected by the remaining zinc.

4 0

3 years ago

When aluminum, AlAl, metal is dipped in an aqueous solution of hydrochloric acid, HClHCl, hydrogen gas, H2H2, is produced with t

kifflom [539]

Answer:

Balanced equation: $2Al(s)+6HCl(aq.)\rightarrow 2AlCl_{3}(aq.)+3H_{2}(g)$

Explanation:

Al is an metallic species with a standard reduction potential of -1.66 V( $E_{Al^{3+}\mid Al}^{0}=-1.66V$ ).
$H_{2}$ is present at the intermediate position in electrochemical series with a standard reduction potential of 0 V ( $E_{H^{+}\mid H_{2}}^{0}=0V$ ).

So, when Al is dipped in aqueous solution of HCl, Al is readily oxidized to produce $Al^{3+}$ whereas $H^{+}$ is reduced to $H_{2}$ .
Hence, as a whole, aqueous $AlCl_{3}$ and gaseous $H_{2}$ is produced as products.

Balanced equation: $2Al(s)+6HCl(aq.)\rightarrow 2AlCl_{3}(aq.)+3H_{2}(g)$

5 0

4 years ago