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3 years ago

URGENT!!-- Please help!

Chemistry

1 answer:

blondinia [14]3 years ago

3 0

Moles of gas = 0.369

<h3>Further explanation</h3>

Given

P = 2 atm

V = 5.3 L

T = 350 L

Required

moles of gas

Solution

Ideal gas Law

$\tt n=\dfrac{PV}{RT}\\\\n=\dfrac{2\times 5.3}{0.082\times 350}\\\\n=0.369$

Avogadro's law : at the same temperature and pressure, the ratio of gas volume will be equal to the ratio of gas moles

moles of O₂ = 45% x 0.369 = 0.166

moles of Ar = 12% x 0.369 = 0.044

moles of N = 43% x 0.369 = 0.159

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<h3>Further explanation</h3>

Given

Reaction

2Fe(s)+3O₂(g)⇒2Fe₂O₃(s)

Required

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Solution

In a balanced chemical equation, the number of atoms in the compound that reacts (the reactants and products) will have the same number

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3 years ago

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Ahat [919]

Answer :

Oxidation number or oxidation state : It represent the number of electrons lost or gained by the atoms of an element in a compound.

Oxidation numbers are generally written with the sign (+) and (-) first and then the magnitude.

Rules for Oxidation Numbers are :

The oxidation number of a free element is always zero.
The oxidation number of a monatomic ion equals the charge of the ion.
The oxidation number of Hydrogen (H) is +1, but it is -1 in when combined with less electronegative elements.
The oxidation number of oxygen (O) in compounds is usually -2.
The oxidation number of a Group 17 element in a binary compound is -1.
The sum of the oxidation numbers of all of the atoms in a neutral compound is zero.
The sum of the oxidation numbers in a polyatomic ion is equal to the charge of the ion.

Now we have to determine the oxidation state of the elements in the compound.

(a) $H_2SO_4$