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2 years ago

In the following equation, is being oxidized and is being reduced.

Chemistry

1 answer:

Mashcka [7]2 years ago

6 0

$oxidation \: number \: of \: oxygen = \\ before \: rxn = - 2 \\ after \: rxn = - 2$

$oxidation \: number \: of \: hydrogen = \\ before \: rxn = + 1 \\ after \: rxn = \\ 2x - 2 = 0 \\ x = + 1$

$oxidation \: number \: of \: carbon = \\ before \: rxn = \\ x - 6 = - 2 \\ x = 4 \\ after \: rxn = \\ x - 4 = 0 \\ x = 4$

<h2>Option A</h2>

$oxidation \: numbers \: remain \: constant \\ so \: none \:a re \: undergoing \: oxidation \: \\ nor \: reduction \:$

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2 years ago

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3 years ago

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ladessa [460]

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For iron:

Given mass of iron = 930 kg = 930000 g (1kg=1000g)

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Putting values in equation 1, we get:

$\text{Moles of iron}=\frac{930000g}{56g/mol}=16607mol$

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By Stoichiometry of the reaction:

2 moles of iron are produced by = 1 mole of $Fe_2O_3$

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Now, calculating the mass of $Fe_2O_3$ from equation 1, we get:

Mass of $Fe_2O_3$ = $moles\times {\text {molar mass}}=8303\times 160=1328480g=1328kg$

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boyakko [2]

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In the following equation, ______ is being oxidized and ______ is being reduced.

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