Nitrogen atomic no.=7
electron=7its electronic configuration =1s2 2s2 2p3
answer: it is true because a hypothesis is something you think will happen during a experiment
explained: I took the test
Answer:
In the given chemical reaction:
Species Oxidized: I⁻
Species Reduced: Fe³⁺
Oxidizing agent: Fe³⁺
Reducing agent: I⁻
As the reaction proceeds, electrons are transferred from I⁻ to Fe³⁺
Explanation:
Redox reaction is a chemical reaction involving the simultaneous movement of electrons thereby causing oxidation of one species and reduction of the other species.
The chemical species that <u><em>gets reduced by gaining electrons </em></u><u>is called an </u><u><em>oxidizing agent</em></u>. Whereas, the chemical species that <u><em>gets oxidized by losing electrons </em></u><u>is called a </u><u><em>reducing agent</em></u><u>.</u>
Given redox reaction: 2Fe³⁺ + 2I⁻ → 2Fe²⁺ + I₂
<u>Oxidation half-reaction</u>: 2 I⁻ + → I₂ + 2 e⁻ ....(1)
<u>Reduction half-reaction</u>: [ Fe³⁺ + 1 e⁻ → Fe²⁺ ] × 2
⇒ 2 Fe³⁺ + 2 e⁻ → 2 Fe²⁺ ....(2)
In the given redox reaction, <u>Fe³⁺ (oxidation state +3) accepts electrons and gets reduced to Fe²⁺ (oxidation state +2) and I⁻ (oxidation state -1) loses electrons and gets oxidized to I₂ (oxidation state 0).</u>
<u>Therefore, Fe³⁺ is the oxidizing agent and I⁻ is the reducing agent and the electrons are transferred from I⁻ to Fe³⁺.</u>
Answer:
MoClBr₂
Explanation:
First we calculate the mass of bromine in the compound:
- 300.00 g - (82.46224 g + 45.741 g) = 171.79676 g
Then we<u> calculate the number of moles of each element</u>, using their <em>respective molar masses</em>:
- 82.46224 g Mo ÷ 95.95 g/mol = 0.9594 mol Mo
- 45.741 g Cl ÷ 35.45 g/mol = 1.290 mol Cl
- 171.79676 g Br ÷79.9 g/mol = 2.150 mol Br
Now we <u>divide those numbers of moles by the lowest number among them</u>:
- 0.9594 mol Mo / 0.9594 = 1
- 1.290 mol Cl / 0.9594 = 1.34 ≅ 1
- 2.150 mol Br / 0.9594 = 2.24 ≅ 2
Meaning the empirical formula is MoClBr₂.
Hydrogen sulfide gas is reacted with dioxygen gas to produce gaseous sulfur dioxide and water. It is false.
When hydrogen sulfide gas reacts with dioxygen gas, it produces water and solid Sulphur and not gaseous sulfur. The chemical equation of the given substances is :
2H2S + O2 → 2S + 2H20
It is a redox reaction as both Oxidation and reduction happens in it. Oxidation of hydrogen sulphur to sulphur happens and reductions of oxygen to water takes place.
if you need to learn more about chemical reaction of Hydrogen sulfide gas, click here
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