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SSSSS [86.1K]
3 years ago
15

PLSS HELP ASAP it's due

Chemistry
1 answer:
BartSMP [9]3 years ago
8 0
<h3>Answer:</h3>

87.02%

<h3>Explanation:</h3>

Percent yield of a product in a chemical equation is the ratio of actual or experimental yield to theoretical yield expressed as percentage.

In this case we are given;

Mass of Zinc as 7.23 g

Actual volume of Hydrogen gas produced as 2.16 L

We are required to calculate the percentage yield of Hydrogen gas;

<h3>Step 1: Write a balanced equation for the reaction</h3>

The balanced equation for the reaction between Zinc metal and Hydrochloric acid is given by;

Zn(s) + 2HCl(aq) → ZnCl₂(aq) + H₂(g)

<h3 /><h3>Step 2: Moles of Zinc metal that reacted </h3>

Moles are given by dividing mass with molar mass

Moles = Mass ÷ Molar mass

Molar mass of Zinc = 65.38 g/mol

Therefore;

Number of moles = 7.23 g ÷ 65.38 g/mol

                             = 0.1106 moles

<h3>Step 3: Calculate the number of moles of Hydrogen gas produced</h3>

From the equation 1 mole of Zinc results in the formation of 1 mole of Hydrogen gas.

Therefore, Moles of hydrogen gas = Moles of Zinc × 1

                                                         = 0.1106 moles × 1

                                                         = 0.1106 moles

<h3>Step 4: Calculate the theoretical volume of Hydrogen gas produced.</h3>

At STP, 1 mole of a gas occupies 22.4 Liters

Therefore;

Volume of Hydrogen = Number of moles × 22.4 L

                                   = 0.1106 mole × 22.4 L

                                  = 2.477 L

<h3>Step 5: Calculate the percent yield </h3>

Percent yield = (Actual yield ÷ Theoretical Yield) × 100%

                      = (2.16 L ÷ 2.477 L)× 100%

                     = 87.20%

Thus, the percent yield of hydrogen gas produced is 87.02%

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