What is the smallest whole-number coefficient for h₂s when the equation h₂s mno₄⁻ → mn²⁺ so₄²⁻ is balanced in acidic solution?
1 answer:
The lowest smallest whole-number coefficient for H₂S is 5. Option C
<h3>What is the smallest whole-number coefficient for H₂S?</h3>Now we know that a redox reaction is one in which there is a loss and gain of electrons One specie is oxidized (looses electrons) while another specie is reduced (gains electrons). The electrons must be transferred leading to an increase in oxidation number of one specie and a decrease in the oxidation number of another.
Now the reduction half equation is;
MnO4^-(aq) + 8H^+(aq) + 5e^- ----> Mn^2+(aq) + 4H2O (l)
The oxidation half equation is;
H2S(aq) ----> S^2-(aq) + 2H^+(aq) + 2e^-
Multiplying the reduction half equation by 2 and the oxidation half equation is 5
2MnO4^-(aq) + 16H^+(aq) + 10e^- ----> 2Mn^2+(aq) + 8H2O (l)
And;
5H2S(aq) ----> 5S^2-(aq) + 10H^+(aq) + 10e^-
The overall balanced reaction equation is;
2MnO4^-(aq) + 6H^+(aq) + 5H2S(aq) ----> 2Mn^2+(aq) + 8H2O (l) + 5S^2-(aq)
Thus the lowest smallest whole-number coefficient for H₂S is 5.
Learn more about redox reaction:brainly.com/question/13293425
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Answer:
<h3>Theanswer is 6 moles</h3>Explanation:
To find the number of moles in a substance given it's number of entities we use the formula
where n is the number of moles
N is the number of entities
L is the Avogadro's constant which is
6.02 × 10²³ entities
From the question we have
We have the final answer as
<h3>6 moles</h3>Hope this helps you
Answer:
See explanation below
Explanation:
In this case, let's see both molecules per separate:
In the case of SeO₂ the central atom would be the Se. The Se has oxidation states of 2+, and 4+. In this molecule it's working with the 4+, while oxygen is working with the 2- state. Now, how do we know that Se is working with that state?, simply, let's do an equation for it. We know that this molecule has a formal charge of 0, so:
Se = x
O = -2
x + (-2)*2 = 0
x - 4 = 0
x = +4.
Therefore, Selenium is working with +4 state, the only way to bond this molecule is with a covalent bond, and in the case of the oxygen will be with double bond. See picture below.
In the case of CO₂ happens something similar. Carbon is working with +4 state, so in order to stabilize the charges, it has to be bonded with double bonds with both oxygens. The picture below shows.
