Isn't it supposed to be MCl4 since the answer is 3.9 , how is it MCl3 ?

Answer 1

It seems like you're discussing a chemical compound denoted as "MCl4" versus "MCl3" in the context of a calculation or a result of 3.9. To provide a more accurate answer, I'd need additional context regarding what the "M" represents, the nature of the calculation, and what "3.9" refers to (e.g., a molarity, a mass, an equilibrium constant, etc.).

In general terms:

• MCl3 implies that metal M forms a trivalent (3+) ion and combines with three chloride ions.
• MCl4 implies that metal M forms a quadrivalent (4+) ion and combines with four chloride ions.

The correct compound can depend on the oxidation state of the metal and its ability to form complexes with chloride ions. Additionally, different stoichiometries can yield different numerical answers in chemical calculations.

If you can provide more details about the chemical system or the specific question you're referring to, I can help clarify the distinction and confirm the correct formula based on the evidence provided.

Answer 2

I worked it like this:

M Cl
6 23.66
_____ _______
35.5. 35.5

=1. =3.9

Answer 3

Thank you for providing the calculation. Let's break down what you have shared.

From your calculation, it looks like you're trying to determine the molar ratio of metal (M) to chlorine (Cl) in a compound using mass percentages or similar values.

In the values you posted:

• \( M \) = 6 (presumably the mass of the metal)
• \( Cl \) = 23.66 (presumably the mass of chlorine)

You used these values and divided them by their respective molar masses (which is 35.5 g/mol for manganese and 23.66 g/mol for Cl, assuming that's what you're using).

From your division, you found:

• For M: \( \frac{6}{35.5} \approx 0.169 \)
• For Cl: \( \frac{23.66}{35.5} \approx 0.67 \)

It seems you're using the ratio of these values to eliminate units by finding a relationship. However, depending on how you've approached the ratios, the final result may lead you to MCl3 or MCl4, depending on the stoichiometric coefficients you derive from your calculation.

Given that you have reached a value of 3.9 through a calculation involving molar masses, it is important to compare the amounts of \[M\] and \[Cl\] in terms of moles to arrive at a conclusion about the stoichiometry of your compound.

Make sure you’re confirming the molar masses you’re using and double-check if you have used mass percentages or actual masses. If MCl3 corresponds to a ratio of 1:3 (M:Cl), and MCl4 corresponds to a ratio of 1:4, the calculated number of moles based on your data should help clarify which compound is correct.

Finally, if you concluded with the formula MCl3 based on a 3.9 factor, it suggests that for every 1 atom of M, there are about 3.9 atoms of Cl. To help, could you clarify what the actual masses or percentages used in your calculations represent? This would help ensure that any confusion about the stoichiometry can be resolved correctly.