Balance the chemical equation given below, and determine the number of grams of MgO are needed to produce 15.0 g of Fe2O3.________ MgO(s) + ________ Fe(s) → ________ Fe2O3(s) + ________ Mg(s)

Answer:Balanced reaction:3MgO + 2Fe -> 3Mg + Fe2O311.3 g of MgO are needed to produce 15 g of Fe2O3Explanation:The balanced reaction is:3MgO + 2Fe -> 3Mg + Fe2O3Ratio is 1:3. First of all we determine the moles of produced oxide.15 g . 1mol / 159.7 g = 0.0939 moles.Now, the rule of three:1 mol of oxide was produced by 3 moles of MgOThen, 0.0939 moles of oxide were produced by 0.282 moles.If we convert the moles to mass, we will get the answer 0.282 mol . 40.3g / 1mol = 11.3 g

Answer:We need 11.35 grams of MgO Explanation:Step 1: Data givenMass of Fe2O3 = 15.0 grams Molar mass Fe2O3 = 159.69 g/molStep 2: The balanced equation3MgO(s) +  2Fe(s) →  Fe2O3(s) + 3Mg(s)Step 3: Calculate moles Fe2O3Moles Fe2O3 = mass Fe2O3 / molar mass Fe2O3 Moles Fe2O3 = 15.0 grams / 159.69 g/molMoles Fe2O3 = 0.0939 molesStep 4: Calculate moles MgOFor 3 moles MgO we need 2 moles Fe to produce 1 mol Fe2O3 and 3 moles MgFor 0.0939 moles Fe2O3 we need 3* 0.0939 = 0.2817 moles MgOStep 5: Calculate mass MgOMass MgO = moles MgO * molar mass MgOMass MgO = 0.2817 moles * 40.30 g/molMass MgO = 11.35 gramsWe need 11.35 grams of MgO