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swat32
3 years ago
13

a quantity of zinc reacts with sulfuric acid and produces 0.10g of hydrogen. how many particles of zinc are required socratic.or

g?
Chemistry
1 answer:
alekssr [168]3 years ago
6 0

Answer:

grams of zinc required = 3.24 g

Particles of zinc required = 2.99\times 10^{22}

Explanation:

Given that:-

Mass of hydrogen gas produced = 0.10 g

Calculation of the moles of H_2 as:-

Mass = 0.10 g

Molar mass of H_2 = 2.016 g/mol

The formula for the calculation of moles is shown below:

moles = \frac{Mass\ taken}{Molar\ mass}

Thus,

Moles= \frac{0.10\ g}{2.016\ g/mol}

Moles= 0.0496\ mol

According to the reaction shown below:-

Zn+H_2SO_4\rightarrow ZnSO_4+H_2

1 mole of hydrogen gas is produced when 1 mole of zinc reacts

So,

0.0496 mole of hydrogen gas is produced when 0.0496 mole of zinc reacts

Moles of Zinc required = 0.0496 moles

Molar mass of zinc = 65.38 g/mol

mass= Moles*Molar mass = 0.0496\ moles\times 65.38\ g/mol=3.24\ g

Also, 1 mole of Zinc contains 6.023\times 10^{23} particles

0.0496 mole of Zinc contains 0.0496\times 6.023\times 10^{23} particles

Particles of zinc required = 2.99\times 10^{22}

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Answer:

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Explanation:

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First we <u>calculate the number of moles of each reactant</u>, using the <em>given volumes and concentrations</em>:

  • 0.75 M Acetic acid * 50.0 mL = 37.5 mmol acetic acid
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We<u> calculate how many acetic acid moles remain after the reaction</u>:

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We now <u>calculate the molar concentration of acetic acid after the reaction</u>:

27.5 mmol / (50.0 mL + 10.0 mL) = 0.458 M

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Finally we <u>calculate the pH</u>:

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