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3 years ago

How many moles are in 2.0 grams of FeO

Chemistry

2 answers:

timurjin [86]3 years ago

7 0

Answer: 0.027837938656318

Explanation: Because 1 grams FeO is equal to 0.013918969328159 mole.

Natali [406]3 years ago

4 0

Answer:

.027798 moles

Explanation:

Molar mass of Iron (II) Oxide.

Molar mass of iron is 55.847

Molar mass of Oxygen is 15.9994

Add the two.

55.947 + 15.9994 = 71.9464

2 (grams) / 71.9464 (molar mass) = .027798 moles

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The iodine "clock reaction" involves the following sequence of reactions occurring in a reaction mixture in a single beaker. 1.

Mars2501 [29]

C: 0.012 mol.

<h3>Explanation</h3>

Start with 0.0020 moles of iodate ions ${\text{IO}_{3}}^{-}$ .

How many moles of iodine $\text{I}_2$ will be produced?

${\text{IO}_{3}}^{-}$ converts to $\text{I}_2$ in the first reaction. The coefficient in front of $\text{I}_2$ is three times the coefficient in front of ${\text{IO}_{3}}^{-}$ . In other words, each mole of ${\text{IO}_{3}}^{-}$ will produce three moles of $\text{I}_2$ . 0.0020 moles of ${\text{IO}_{3}}^{-}$ will convert to 0.0060 moles of $\text{I}_2$ .

How many moles of thiosulfate ions ${\text{S}_2\text{O}_3}^{2-}$ are required?

$\text{I}_2$ reacts with ${\text{S}_2\text{O}_3}^{2-}$ in the second reaction. The coefficient in front of $\text{I}_2$ is twice the coefficient in front of ${\text{S}_2\text{O}_3}^{2-}$ . How many moles of ${\text{S}_2\text{O}_3}^{2-}$ does each mole of $\text{I}_2$ consume? Two. 0.0060 moles of $\text{I}_2$ will be produced. As a result, $2 \times 0.0060 = 0.0120$ moles of ${\text{S}_2\text{O}_3}^{2-}$ will be needed.

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3 years ago

If a container contains 3.5 moles and has a volume of 1.5 L, then what volume is it when it contains 8 moles? *

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Explanation:

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