Arkadaşlar kimya hakkında hiçbir bilgim yok lütfen emin olanlar cevaplasın :))

How do you find the charge of an ion

I am Lyosha [343]

Answer: To find the charge of an ion you must add the charge of protons and charge of electrons of an element.

Explanation: By doing this you get the overall charge of the ion.

6 0

3 years ago

Water vapor is heated and rising into the air is called what?

Lady_Fox [76]

Answer:

Evaporation

Explanation:

3 0

3 years ago

Which of the following elements has 3 electrons in the 2p sublevel?

Arlecino [84]

Answer:

the answer is D. N

AP3X

8 0

3 years ago

If 588 grams of FeS2 is allowed to react with 352 grams of O2 according to the following equation, how many grams of Fe2O3 are p

Rainbow [258]

Answer: The mass of iron (III) oxide produced is 782.5 grams

Explanation:

To calculate the number of moles, we use the equation:

$\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}$ .....(1)

For $FeS_2$ :

Given mass of $FeS_2$ = 588 g

Molar mass of $FeS_2$ = 120 g/mol

Putting values in equation 1, we get:

$\text{Moles of }FeS_2=\frac{588g}{120g/mol}=4.9mol$

For $O_2$ :

Given mass of $O_2$ = 352 g

Molar mass of $O_2$ = 32 g/mol

Putting values in equation 1, we get:

$\text{Moles of }O_2=\frac{352g}{32g/mol}=11mol$

The chemical equation for the reaction of $FeS_2$ and oxygen gas follows:

$FeS_2+O_2\rightarrow Fe_2O_3+SO_2$

By Stoichiometry of the reaction:

1 mole of $FeS_2$ reacts with 1 mole of oxygen gas

So, 4.9 moles of $FeS_2$ will react with = $\frac{1}{1}\times 4.9=4.9mol$ of oxygen gas

As, given amount of oxygen gas is more than the required amount. So, it is considered as an excess reagent.

Thus, $FeS_2$ is considered as a limiting reagent because it limits the formation of product.

By Stoichiometry of the reaction:

1 mole of $FeS_2$ produces 1 mole of iron (III) oxide

So, 4.9 moles of $FeS_2$ will produce = $\frac{1}{1}\times 4.9=4.9moles$ of iron (III) oxide

Now, calculating the mass of iron (III) oxide from equation 1, we get:

Molar mass of iron (III) oxide = 159.7 g/mol

Moles of iron (III) oxide = 4.9 moles

Putting values in equation 1, we get:

$4.9mol=\frac{\text{Mass of iron (III) oxide}}{159.7g/mol}\\\\\text{Mass of iron (III) oxide}=(4.9mol\times 159.7g/mol)=782.5g$

Hence, the mass of iron (III) oxide produced is 782.5 grams

8 0

3 years ago

Write the formula for the complex ion formed by the metal ion Cr3+ and six NO2- ions as ligands. Decide whether the complex coul

Dmitrij [34]

Answer:The metal complex formed would have the following formula [Cr(NO₂)₆]³⁻. The complex has a net negative charge and hence it can only be isolated as a salt with a positive cation so the formed complex could be isolated as potassium salt. The formula for salt would be K₃[Cr(NO₂)₆].

Explanation:

The metal ion given to us is Cr³⁺ (Chromium) in +3 oxidation state.

The electronic configuration for the metal ion is [Ar]3d³ so there are vacant 3d metal orbitals which are available and hence 6 NO₂⁻ ligands can easily attack the metal center and form a metal complex.

The charge on the overall complex can be calculated using the oxidation states of metal and ligand which is provided.

The (chromium ) Cr³⁺ metal has +3 charge and 6 NO₂⁻ (nitro) ligands have -6 charge and since the ligands will be providing a total of 6 - (negative) charge and hence only 3- (negative ) charge can be neutralized so a net 3- negative charge would be present on the overall complex which is basically present at the metal center :

charge on the complex=+3-6=-3

Let X be the Oxidation state of Cr in complex =[Cr(NO₂)₆]³⁻

X-6=-3

X=-3+6

X=+3

so our calculated oxidation state of Cr is +3 which matches with the provided in question.

As we can see that the overall metal complex has a net negative charge and hence and only positively charged cations can form a salt with this metal complex and hence only potassium K⁺ ions can form salt with the metal complex.

since overall charge present on the metal complex is -3 so 3 K⁺ ion would be needed to neutralize it and hence the formula of the metal salt would be K₃[Cr(NO₂)₆].

3 0

3 years ago

Arkadaşlar kimya hakkında hiçbir bilgim yok lütfen emin olanlar cevaplasın :))​

Arkadaşlar kimya hakkında hiçbir bilgim yok lütfen emin olanlar cevaplasın :))