6. How many moles of calcium oxide will be produced when 1.6 moles of iron (III) oxide reacts with calcium phosphate according to the following (unbalanced reaction: underline ( )Fe_(2)O_(3)+underline ( )Ca_(3)(PO_(4))_(2)arrow underline ( )Fe(PO_(4))+underline ( )CaO

Question

6. How many moles of calcium oxide will be produced when 1.6 moles of iron (III) oxide reacts with calcium phosphate according to the following (unbalanced reaction: underline ( )Fe_(2)O_(3)+underline ( )Ca_(3)(PO_(4))_(2)arrow underline ( )Fe(PO_(4))+underline ( )CaO

Answer 1

To determine the number of moles of calcium oxide (CaO) produced when 1.6 moles of iron(III) oxide (Fe2O3) reacts with calcium phosphate (Ca3(PO4)2), we need to first balance the chemical equation.Balanced chemical equation:2 Fe2O3 + 3 Ca3(PO4)2 → 6 Fe(PO4) + 9 CaOFrom the balanced equation, we can see that 2 moles of Fe2O3 produce 9 moles of CaO.Now, we can use the stoichiometric relationship to calculate the number of moles of CaO produced when 1.6 moles of Fe2O3 reacts.Using the stoichiometric relationship:9 moles of CaO / 2 moles of Fe2O3 = x moles of CaO / 1.6 moles of Fe2O3Solving for x:x = (9 moles of CaO / 2 moles of Fe2O3) * 1.6 moles of Fe2O3x = 7.2 moles of CaOTherefore, 7.2 moles of calcium oxide (CaO) will be produced when 1.6 moles of iron(III) oxide (Fe2O3) reacts with calcium phosphate (Ca3(PO4)2).

Problemas

6. How many moles of calcium oxide will be produced when 1.6 moles of iron (III) oxide reacts with calcium phosphate according to the following (unbalanced reaction: underline ( )Fe_(2)O_(3)+underline ( )Ca_(3)(PO_(4))_(2)arrow underline ( )Fe(PO_(4))+underline ( )CaO

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