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MrMuchimi
2 years ago
12

Does anyone know how to do this?

Chemistry
1 answer:
mr Goodwill [35]2 years ago
4 0

Answer:

this look hard

Explanation:

hmm

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Which best explains the statement "It has no definite volume”?
NeX [460]
The correctanswer is D hope this helps
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3 years ago
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Is the sun typical of these nearby stars
marshall27 [118]
No the sun is the biggest star in the universe.
8 0
3 years ago
What is the oxidation number of cl− in the hypochlorite ion clo−?
mariarad [96]

Answer : The oxidation number of chlorine (Cl) is, (+1)

Explanation :

Oxidation number : It represent the number of electrons lost or gained by the atoms of an element in a compound.

Oxidation numbers are generally written with the sign (+) and (-) first and then the magnitude.

When the atoms are present in their elemental state then the oxidation number will be zero.

Rules for Oxidation Numbers :

The oxidation number of a free element is always zero.

The oxidation number of a monatomic ion equals the charge of the ion.

The oxidation number of  Hydrogen (H)  is +1, but it is -1 in when combined with less electronegative elements.

The oxidation number of  oxygen (O)  in compounds is usually -2, but it is -1 in peroxides.

The oxidation number of a Group 1 element in a compound is +1.

The oxidation number of a Group 2 element in a compound is +2.

The oxidation number of a Group 17 element in a binary compound is -1.

The sum of the oxidation numbers of all of the atoms in a neutral compound is zero.

The sum of the oxidation numbers in a polyatomic ion is equal to the charge of the ion.

The given compound is, ClO^-

Let the oxidation state of 'Cl' be, 'x'

x+(-2)=-1\\\\x-2=-1\\\\x=+1

Therefore, the oxidation number of chlorine (Cl) is, (+1)

5 0
3 years ago
2.00 L of 0.800 M NaNO3 must be prepared from a solution known to be 2.50 M in concentration.How many mL are required? Plus don'
Morgarella [4.7K]

Answer:

1.36 × 10³ mL of water.

Explanation:

We can utilize the dilution equation. Recall that:

\displaystyle M_1V_1= M_2V_2

Where <em>M</em> represents molarity and <em>V</em> represents volume.

Let the initial concentration and unknown volume be <em>M</em>₁ and <em>V</em>₁, respectively. Let the final concentration and required volume be <em>M</em>₂ and <em>V</em>₂, respectively. Solve for <em>V</em>₁:

\displaystyle \begin{aligned} (2.50\text{ M})V_1 &= (0.800\text{ M})(2.00\text{ L}) \\ \\ V_1 & = 0.640\text{ L} \end{aligned}

Therefore, we can begin with 0.640 L of the 2.50 M solution and add enough distilled water to dilute the solution to 2.00 L. The required amount of water is thus:
\displaystyle 2.00\text{ L} - 0.640\text{ L} = 1.36\text{ L}

Convert this value to mL:
\displaystyle 1.36\text{ L} \cdot \frac{1000\text{ mL}}{1\text{ L}} = 1.36\times 10^3\text{ mL}

Therefore, about 1.36 × 10³ mL of water need to be added to the 2.50 M solution.

8 0
2 years ago
C) If 0.66 mole of iron (III) oxide were produced from the reaction, that must mean that how many mole
Fudgin [204]

Answer:

If there is 0.66 moles of iron(III)oxide produced, there reacte 0.99 moles of oxygen (O2)

Explanation:

Step 1: Data given

Number of moles iron (III) oxide (Fe2O3) = 0.66 moles

Step 2: The balanced equation

4Fe + 3O2 → 2Fe2O3

Step 3: Calculate moles of oxygen (O2)

For 4 moles Fe consumed, we need 3 moles of O2 to produce 2 moles of Fe2O3

For 0.66 moles Fe2O3 produced, we need 3/2 * 0.66 = 0.99 moles of O2

If there is 0.66 moles of iron(III)oxide produced, there reacte 0.99 moles of oxygen (O2)

4 0
3 years ago
Read 2 more answers
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