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2 years ago

PLEASE HELP ITS FINAL EXAMS!

Chemistry

1 answer:

Maksim231197 [3]2 years ago

7 0

From the stoichiometry of the reaction, 1 mole of ammonia, is produced.

<h3>What is reaction?</h3>

A chemical reaction involves the combination of two or more substances to yield products.

The chemical reaction is; Mg3N₂(s) + 6H₂O(1)→ 2NH3(aq) + 3Mg(OH)2(s)

Number of moles of water = 54.0 g/18 g/mol = 3 moles

Now;

6 moles of water produced 2 moles of ammonia

3 moles of water will produce 3 moles * 2 moles/6 moles

= 1 mole of ammonia

Learn more about reaction:brainly.com/question/17434463

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<u>Answer:</u> The mass of hydrogen cyanide formed is 0.17 grams

<u>Explanation:</u>

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

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

Given mass of KCN = 0.420 g

Molar mass of KCN = 65.12 g/mol

Putting values in equation 1, we get:

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The given chemical equation follows:

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As, hydrochloric acid is present in excess. So, it is considered as an excess reagent.

Thus, potassium cyanide is a limiting reagent because it limits the formation of products.

By Stoichiometry of the reaction:

1 mole of potassium cyanide produces 1 mole of hydrogen cyanide.

So, 0.0064 moles of potassium cyanide will produce = $\frac{1}{1}\times 0.00064=0.0064mol$ of hydrogen cyanide

Now, calculating the mass of hydrogen cyanide from equation 1, we get:

Molar mass of HCN = 27.02 g/mol

Moles of HCN = 0.0064 moles

Putting values in equation 1, we get:

$0.0064mol=\frac{\text{Mass of HCN}}{27.02g/mol}\\\\\text{Mass of HCN}=0.17g$

Hence, the mass of hydrogen cyanide formed is 0.17 grams

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