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Assoli18 [71]
3 years ago
14

What are the respective central-metal oxidation state, coordination number, and overall charge on the complex ion in Na2[Cr(NH3)

2 (NCS)4]?
Chemistry
1 answer:
Elden [556K]3 years ago
6 0

Answer:

Central-metal oxidation state: +2

Coordination number: 6

Overall charge: -2

Explanation:

In the ion complex:

Na₂[Cr(NH₃)₂(NCS)₄]

The central-metal is Cr, the ligands are NH₃ and NCS.

The NH₃ is a neutral ligand, while NCS is an anionic ligand with -1 in charge.

The overall charge of the complex is:

2Na⁺ +  [Cr(NH₃)₂(NCS)₄]⁻² → <em>-2</em>

As NCS gives -1 in charge and there are four NCS, The Cr must be in <em>+2</em> of oxidation state to give an overall charge of -2.

As Cr is bonded to 2 NH₃ and 4 NCS, the coordination number is 2+4 = <em>6</em>

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I hope it helps!

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Identify the parts of the energy diagrams.
Lapatulllka [165]
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Energy release is exothermic reaction whiles energy absorb is endothermic reaction

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What is oxidized and what is reduced <br> C2H4 + 2O2 → 2CO + 2H2O<br> C2H4 + 3O2 → 2CO2 + 2H2O
Anika [276]

C2H4 is oxidized and O2 is reduced in both reactions.

<h3>What is oxidation/reduction?</h3>

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Reduction, on the other hand, is defined as:

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In the two reactions, oxygen is being added to C2H4. Thus, C2H4 is being oxidized.

The oxidizing agent is O2. In oxidation reactions, the oxidizing agents usually get reduced. Thus, O2 is reduced in both reactions.

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Which statement is correct about the rate of a chemical reaction? (5 points)
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1.5mol C3H8 from C3H8+5O2--&gt;3CO2+4H2O .how many grams of carbon dioxide are produced
koban [17]

Answer:

\large \boxed{\text{200 g CO}_{{2}}}

Explanation:

We will need a balanced equation with masses, moles, and molar masses, so let’s gather all the information in one place.

Mᵣ:                                 44.01

            C₃H₈ + 5O₂ ⟶ 3CO₂ + 4H₂O

n/mol:    1.5

1. Calculate the moles of CO₂

The molar ratio is 3 mol  CO₂:1 mol C₃H₈

\rm  \text{Moles of CO}_{2} = \text{1.5 mol C$_{3}$H}_{8} \times \dfrac{\text{3 mol CO}_{2}}{\text{1 mol C$_{3}$H}_{8}} =\text{4.5 mol CO}_{2}

2. Calculate the mass of CO₂.

\text{Mass of CO}_{2} = \text{4.5 mol CO}_{2}  \times \dfrac{\text{44.01 g CO}_{2}}{\text{1 mol CO$_{2}$}} = \textbf{200 g CO}_{\mathbf{2}}\\\text{The reaction will form $\large \boxed{\textbf{200 g CO}_{\mathbf{2}}}$}

3 0
3 years ago
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