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3 years ago

I need help can someone help me

Chemistry

1 answer:

Arisa [49]3 years ago

6 0

Answer:

Option D. The number of oxygen atom is the same before and after the reaction.

Explanation:

From the question given above, the following were obtained:

Robin's equation:

H₂ + O₂ —> H₂O

Alex's equation

2H₂ + O₂ —> 2H₂O

To know which equation better represents the reaction, we shall determine which of the equation is balanced.

For Robin:

H₂ + O₂ —> H₂O

Element >>> Reactant >>> Product

H >>>>>>>>> 2 >>>>>>>>>> 2

O >>>>>>>>> 2 >>>>>>>>>> 1

Robin's equation is not balanced because the number of atoms of each element in the reactant and product are not equal.

For Alex:

2H₂ + O₂ —> 2H₂O

Element >>> Reactant >>> Product

H >>>>>>>>> 4 >>>>>>>>>> 4

O >>>>>>>>> 2 >>>>>>>>>> 2

Alex' equation is balanced because the number of atoms of each element in the reactant and product are equal.

Thus, option D gives the right answer to the question.

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b. Moles of water formed: 1.34 mol

c. Mass of water formed: 24.1 g

d. Mass of oxygen formed: 21.4 g

Explanation:

Dihdyrogen dioxide is the chemical name for a compound made of two hydrogen atoms and two oxide atoms, i.e. H₂O₂, which is also known as hydrogen peroxide or oxygenated water.

The decomposition reaction of dihydrogen dioxide into water and oxygen gas is represented by the balanced chemical equation:

$2H_2O_2(l)\rightarrow 2H_2O(l)+O_2(g)$

The mole ratios derived from that balanced chemical equation are:

2 mol H₂O₂ : 2 mol H₂O : 1 mol O₂

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Set the proportion using the theoretical mole ratio of H₂O₂ to O₂ and the amount of moles of dyhydrogen dioxide that react:

$2\text{ mol }H_2O_2/1\text{ mol }O_2=1.34\text{ mol }H_2O_2/x$

When you solve for x, you get:

x = 1.34 mol H₂O₂ × 1 mol O₂ / 2 mol H₂O₂ = 0.670 mol O₂

b. Moles of water formed

Set the proportion using the theoretical mole ratio of H₂O₂ to H₂O and the amount of moles of dyhydrogen dioxide that react:

$2\text{ mol }H_2O_2/2\text{ mol }H_2O=1.34\text{ mol }H_2O_2/x$

When you solve for x, you get:

x = 1.34 mol H₂O₂ × 2 mol H₂O / 2 mol H₂O₂ = 1.34 mol H₂O

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Using the number of moles of water calculated in the part b., you calculate the mass of water formed, in grams, using the molar mass of water:

Molar mass of water = 18.015 g/mol

Number of moles = mass in grams / molar mass

⇒ mass in grams = number of moles × molar mass

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Using the number of moles of oxygen determined in the part a., you calculate the mass in grams using the molar mass of O₂.

Molar mass of O₂ = 32.00 g/mol

mass = molar mass × number of moles

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