In the reaction #"FeC"l_2 + 2"NaOH" -> "Fe(OH)"_2"(s)" + 2"NaC"l#, if 6 moles of #"FeC"l_2# are added to 6 moles of #"NaOH"#, how many moles of #"FeC"l_2# would be used up in the reaction?
The balanced chemical equation indicates the ratio that must constantly exist between the reactants in any chemical reaction.
As for you, you've
The stoichiometric coefficients for sodium hydroxide and iron(II) chloride, respectively, indicate the mole ratio that needs to be present for this reaction to occur.
Calculate the number of moles of iron(II) chloride that will react with the moles of sodium hydroxide using the previously mentioned mole ratio.
Thus, one could say that
It is evident that all of the sodium hydroxide is used up before any moles of iron(II) chloride have an opportunity to participate in the reaction.
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In the balanced chemical equation ( \text{FeCl}_2 + 2\text{NaOH} \rightarrow \text{Fe(OH)}_2(s) + 2\text{NaCl} ), one mole of ( \text{FeCl}_2 ) reacts with two moles of ( \text{NaOH} ). Therefore, if 6 moles of ( \text{FeCl}_2 ) are added, they would react completely with 12 moles of ( \text{NaOH} ). Hence, all 6 moles of ( \text{FeCl}_2 ) would be used up in the reaction.
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When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
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