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3 years ago

How much iron can be recovered from 25 grams of Fe2O3

Chemistry

2 answers:

Scilla [17]3 years ago

3 0

25.0g of Fe2O3. 2(55.8)g+3(16.0)g=159.9g. 2(55.8)g/159.6g•100%= 69.9%. 69.9%/100%•25.0g=17.5g of iron recovered

Radda [10]3 years ago

3 0

Answer: The mass of iron recovered is 17.5 grams

Explanation:

We are given a chemical compound having chemical formula of $Fe_2O_3$

We know that:

Molar mass of iron (III) oxide = 159.7 g/mol

Mass of iron = 55.8 g/mol

We are given:

Mass of iron (III) oxide = 25 g

To calculate the mass of iron recovered in given amount of iron (III) oxide, we use unitary method:

From 159.7 grams of iron (III) oxide, mass of iron recovered is $(2\times 55.8)g$

So, from 25 grams of iron (III) oxide, mass of iron recovered will be $\frac{(2\times 55.8)}{159.7}\times 25=17.5g$

Hence, the mass of iron recovered is 17.5 grams

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Answer:

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2 years ago

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zhannawk [14.2K]

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2 years ago

If 12.1 kilograms of al2o3(s), 60.4 kilograms of naoh(l), and 60.4 kilograms of hf(g) react completely, how many kilograms of cr

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n(Al₂O₃) = m(Al₂O₃) ÷ M(Al₂O₃).
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3 years ago

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2 years ago

A chemist must prepare of sodium hydroxide solution with a pH of at . He will do this in three steps: Fill a volumetric flask ab

77julia77 [94]

Answer:

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Explanation:

pH value is not provided, so we'll solve this problem in a general case and then we will use an example to justify it.

By definition, $pH = -log[H_3O^+]$ .
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From the equation above, using stoichiometry we can tell that the molarity of hydroxide is equal to the molarity of NaOH: $[NaOH] = [OH^-]$ .
Concentration of hydroxide is then equal to the ratio of moles of NaOH and the volume of the given solution. Moles themselves are equal to mass over molar mass, so we obtain: $[OH^-] = [NaOH] = \frac{n_{NaOH}}{V} = \frac{m_{NaOH}}{M_{NaOH}V}$ .
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