Cuantas moléculas de oxigeno se producen por la descomposición de 28.5 g de H2O2 (masa molecular = 34.0g/mol) de acuerdo a la ecuación 2H2O2(l) → 2H2O(l)+O2(g)

Answers

Answer 1

Answer:

The question is as follows: How many oxygen molecules are produced by the decomposition of 28.5 g of H2O2 (molecular mass = 34.0g / mol) according to the equation

2H2O2 (l) → 2H2O (l) + O2 (g)

Answer: There are $2.52 * 10^(23)$ molecules are produced by the decomposition of 28.5 g of $H_(2)O_(2)$ according to the equation $2H_(2)O(l) \rightarrow 2H_(2)O(l) + O_(2)(g)$ .

Explanation:

Given: Mass of $H_(2)O_(2)$ = 28.5 g

As moles is the mass of a substance divided by its molar mass. Hence, moles of $H_(2)O_(2)$ is calculated as follow.

$Moles = (mass)/(molarmass)\n= (28.5 g)/(34.0 g/mol)\n= 0.838 mol$

According to the given equation, 2 moles of $H_(2)O_(2)$ gives 1 mole of $O_(2)$ . So, moles of $O_(2)$ produced by 0.838 moles of $H_(2)O_(2)$ will be calculated as follows.

$Moles of O_(2) = (0.838 mol)/(2)\n= 0.419 mol$

This means that moles of $O_(2)$ produced is 0.419 mol.

As per the mole concept, 1 mole of every substance has $6.022 * 10^(23)$ molecules.

So, molecules of $O_(2)$ present in 0.419 mole are as follows.

$0.419 * 6.022 * 10^(23)\n= 2.52 * 10^(23)$

Thus, we can conclude that there are $2.52 * 10^(23)$ molecules are produced by the decomposition of 28.5 g of $H_(2)O_(2)$ according to the equation $2H_(2)O(l) \rightarrow 2H_(2)O(l) + O_(2)(g)$ .

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Answers

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Answers

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Answers

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Answers

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