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Iron metal reacts with chlorine gas giving iron(III) chloride. The balanced chemical equation for this reaction is: 2 Fe(s) + 3 Cl2(g) โ†’ 2 FeCl3(s). Beginning with 43.0 g of iron, what mass of Cl2, in grams, is required for the complete reaction? What mass of FeCl3 can be produced?

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Coleen Amado
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26 Dec 2020

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Related questions

Iron metal reacts with chlorine gas giving iron (III) chloride. The balanced chemical equation for this reaction is:

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Beginning with of iron, what mass of , in grams, is required for complete reaction?

What mass of can be produced?

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Consider the reaction: Fe(s)+Cl2(g)รขย†ย’FeCl3(s). How many moles of chlorine gas react with 0.180 mol of metallic iron and How many moles of iron(III) chloride are produced?

Iron reacts with chlorine gas to form iron (III) chloride. Given this, answer the following.

(a) What is the balanced chemical reaction?

(b) Given 10.0 g of iron, what mass, in grams, of chlorine gas would be required to complete the reaction?

(c) If only 18.5 g of FeCl3 is formed from 10.0 g of iron and excess chlorine gas, what is the percent yield of the reaction?

(d) If 10.0 g each of iron and chlorine gas are combined, what is the theoretical yield of iron (III) chloride?

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