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3 years ago

Consider the following equilibrium

Chemistry

2 answers:

Alex73 [517]3 years ago

8 0

Answer:

Which statement about this system is true?

✔ The equilibrium lies to the left.

If the equilibrium concentration of NO2 is 1.78 × 10–2 M, the equilibrium concentration of N2O4 is

✔ 5.42 × 10⁻² M.

Explanation:

goldfiish [28.3K]3 years ago

3 0

Answer:

uploa

Explanation:

uploaded to the nearest inch and the same for the miscommunication between the two of the three

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Write a balanced half-reaction for the reduction of dichromate ion to chromium ion in acidic aqueous solution. Be sure to add ph

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Answer:

The balanced half-reaction for the reduction of dichromate ion to chromium ion in acidic aqueous solution:

$Cr_2O_7^{2-}(aq)+14H^+(aq)+6e^-\rightarrow 2Cr^{3+}(aq)+7H_2O(l)$

Explanation:

The reaction :

$Cr_2O_7^{2-}\rightarrow Cr^{3+}$

Balancing of reaction in an acidic medium:

Step 1: Balance the atoms in the reaction:

$Cr_2O_7^{2-}(aq)\rightarrow 2Cr^{3+}(aq)$

Step 2: Balance oxygen atom by adding water on the side where no oxygen or less oxygen atom is present;

$Cr_2O_7^{2-}(aq)\rightarrow 2Cr^{3+}(aq)+7H_2O(l)$

Step 3: Balance the hydrogen atom by adding hydrogen ions on the side where water is absent:

$Cr_2O_7^{2-}(aq)+14H^+(aq)\rightarrow 2Cr^{3+}(aq)+7H_2O(l)$

Step 4: Now balance charge by adding electrons on the side where more positive charge is present

$Cr_2O_7^{2-}(aq)+14H^+(aq)+6e^-\rightarrow 2Cr^{3+}(aq)+7H_2O(l)$

The balanced half-reaction for the reduction of dichromate ion to chromium ion in acidic aqueous solution:

$Cr_2O_7^{2-}(aq)+14H^+(aq)+6e^-\rightarrow 2Cr^{3+}(aq)+7H_2O(l)$

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