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2 years ago

5. In a general chemistry laboratory experiment, a student produces 2.73 g of a compound. She calculates the

1 answer:

8 0

The percent yield is given by the actual and the theoretical yield. The percent yield of the 2.73 gm compound is 80.3%. Thus, option b is correct.

<h3>What is the percent yield?</h3>

The percent yield is the ratio of the actual yield to the theoretical yield. It is calculated as:

% Yield = Actual yield ÷ Theoretical yield × 100%

= 2.73 ÷ 3.84 × 100%

= 71.09 %

As the closest number to 71.09 is 80.3% the percent yield will be 80.3%.

There is no limiting reagent in the reaction between the copper iodide and mercury iodide as the moles of the reactants and the products are in equal quantity.

Hence, option b. there is no limiting reagent in this reaction.

Learn more about percent yield here:

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Explain the difference between the reacts and products of a chemical reaction

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3 years ago

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Does the wave require a medium in order to travel?

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3 years ago

What is the reduction half-reaction for the equation below?

Katen [24]

Answer:

$MnO_4^-+8H^++5e^-\rightarrow Mn^{2+}+4H_2O$

Explanation:

Hello there!

In this case, since redox reactions are characterized by the presence of a reduction reaction, whereby the oxidation of the element decreases, and an oxidation reaction whereby the oxidation of the element increases.

In such a way, for the given chemical equation, we can see Fe is increasing its oxidation state from 2+ to 3+, which means it is oxidized. On the flip side, Mn is being reduced from 7+ (MnO₄⁻) to 2+ and this, the reduction half-reaction is:

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Regards!

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3 years ago