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How many moles of iron can be produced from the reaction of 10 mol Fe2O3 and 25 mol of CO?
From the balanced chemical equation 3Fe2O3 + CO → 2Fe3O4 + CO2, it can be seen that 3 moles of Fe2O3 react with 1 mole of CO to produce 2 moles of Fe. Therefore, if 25 moles of CO react, it will produce 25/3 * 2 = 16.67 moles of Fe.
If 4.00 kg of Fe2O3 are available to react how many moles of CO are needed and how many moles of each product are formed?
mass / molar mass molar mass Fe2O3 = 159.69 g/mol mass Fe2)3 = 4.00 kg = 4000 g moles = 4000 g / 159.69 g/mol = 25.05 moles Fe2O3 The balanced equation tells you that 1 mole Fe2O3 requires 3 moles CO to react So 25.05 moles needs (3 x 25.05) moles CO = 75.15 moles Co is needed to react 4.00 kg Fe2O3 = 75.2 mol (3 sig figs) b) The equation tells you that 1 moles Fe2O3 reacts to form 2 moles Fe So 25.05 moles will form (2 x 25.05) mol Fe moles Fe formed = 50.10 moles = 50.1 mol (3 sig figs) The equation tells you 1 mole Fe2O3 reacts to form 3 moles CO2 So 25.05 mol Fe2O3 will form (3 x 25.05) mol CO2 = 75.15 moles CO2 = 75.2 mol (3 sig figs) ==
How many grams of CO react with .390 kg of Fe2O3?
Fe2O3 (s) + 3 CO (g) 🡪 2 Fe (s) + 3 CO2 (g) Calculate the number of grams of CO that can react with 250 g of Fe2O3. Calculate the number of grams of Fe and the number of grams of CO2 formed when 250 grams of Fe2O3 reacts.
Which statement is true if 12 mol co and 12 mol fe2o3 are allowed to react?
If 12 mol of CO and 12 mol of Fe2O3 are allowed to react, the limiting reactant will be CO. The balanced chemical equation is 3CO + Fe2O3 -> 2Fe + 3CO2, and since it takes 3 mol of CO to react with 1 mol of Fe2O3, there is excess Fe2O3 left after the CO is consumed.
How many grams of C are required to react with 2.50 moles of Fe2O3?
To determine the grams of carbon needed to react with 2.50 moles of Fe2O3, you first need to balance the equation for the reaction between C and Fe2O3. Then, calculate the molar ratio between C and Fe2O3 from the balanced equation. Finally, use the molar mass of carbon to convert the moles of carbon to grams.
How many grams of CO are needed to react with 3.16 g of Fe2O3?
To calculate the grams of CO needed to react with Fe2O3, you need to write a balanced chemical equation for the reaction, determine the moles of Fe2O3 given the mass provided, and use the stoichiometry of the balanced equation to find the moles of CO needed. Finally, convert the moles of CO to grams using the molar mass of CO.
How many moles of iron can be produced from the reaction of 10 mol Fe2O3 and 25 mol of CO?
From the balanced chemical equation 3Fe2O3 + CO → 2Fe3O4 + CO2, it can be seen that 3 moles of Fe2O3 react with 1 mole of CO to produce 2 moles of Fe. Therefore, if 25 moles of CO react, it will produce 25/3 * 2 = 16.67 moles of Fe.
If 4.00 kg of Fe2O3 are available to react how many moles of CO are needed and how many moles of each product are formed?
mass / molar mass molar mass Fe2O3 = 159.69 g/mol mass Fe2)3 = 4.00 kg = 4000 g moles = 4000 g / 159.69 g/mol = 25.05 moles Fe2O3 The balanced equation tells you that 1 mole Fe2O3 requires 3 moles CO to react So 25.05 moles needs (3 x 25.05) moles CO = 75.15 moles Co is needed to react 4.00 kg Fe2O3 = 75.2 mol (3 sig figs) b) The equation tells you that 1 moles Fe2O3 reacts to form 2 moles Fe So 25.05 moles will form (2 x 25.05) mol Fe moles Fe formed = 50.10 moles = 50.1 mol (3 sig figs) The equation tells you 1 mole Fe2O3 reacts to form 3 moles CO2 So 25.05 mol Fe2O3 will form (3 x 25.05) mol CO2 = 75.15 moles CO2 = 75.2 mol (3 sig figs) ==
How many grams of CO react with .390 kg of Fe2O3?
Fe2O3 (s) + 3 CO (g) 🡪 2 Fe (s) + 3 CO2 (g) Calculate the number of grams of CO that can react with 250 g of Fe2O3. Calculate the number of grams of Fe and the number of grams of CO2 formed when 250 grams of Fe2O3 reacts.
Which statement is true if 12 mol co and 12 mol fe2o3 are allowed to react?
If 12 mol of CO and 12 mol of Fe2O3 are allowed to react, the limiting reactant will be CO. The balanced chemical equation is 3CO + Fe2O3 -> 2Fe + 3CO2, and since it takes 3 mol of CO to react with 1 mol of Fe2O3, there is excess Fe2O3 left after the CO is consumed.
How many grams of C are required to react with 2.50 moles of Fe2O3?
To determine the grams of carbon needed to react with 2.50 moles of Fe2O3, you first need to balance the equation for the reaction between C and Fe2O3. Then, calculate the molar ratio between C and Fe2O3 from the balanced equation. Finally, use the molar mass of carbon to convert the moles of carbon to grams.
How many moles of Fe2O3 are necessary to produce 0.824 mol of CO2?
To determine how many moles of Fe2O3 are required to produce 0.824 moles of CO2, we first need to look at the balanced chemical reaction involved in the process. In the reduction of iron(III) oxide (Fe2O3) with carbon (C), the reaction can be represented as: [ \text{Fe}_2\text{O}_3 + 3\text{C} \rightarrow 2\text{Fe} + 3\text{CO} ] In this reaction, 1 mole of Fe2O3 produces 3 moles of CO. Since CO2 is produced from the combustion of CO, we need to convert CO to CO2. However, the stoichiometry from Fe2O3 to CO directly leads us to find that 1 mole of Fe2O3 results in the generation of 3 moles of CO, which can then produce CO2. Thus, to produce 0.824 moles of CO2, we will need to calculate based on the conversion of moles of CO to CO2 (1:1 ratio). Therefore, we need: [ \text{Moles of Fe}_2\text{O}_3 = \frac{0.824 , \text{mol CO2}}{3 , \text{mol CO}} \approx 0.2747 , \text{mol Fe2O3} ] Thus, approximately 0.275 moles of Fe2O3 are needed to produce 0.824 moles of CO2.
How many moles of oxygen would be needed to react with 4.52 moles of CO?
To determine the number of moles of oxygen needed to react with 4.52 moles of carbon monoxide (CO), we refer to the balanced chemical equation for the reaction: 2 CO + O₂ → 2 CO₂. From the equation, 2 moles of CO react with 1 mole of O₂. Therefore, to find the moles of O₂ required, we can use the ratio: (4.52 moles CO) × (1 mole O₂ / 2 moles CO) = 2.26 moles of O₂. Thus, 2.26 moles of oxygen are needed to react with 4.52 moles of CO.
What are some parts of a chemical change?
Depict moles eg: Fe2O3(s) + 3CO(g)--> 2Fe(s) + 3CO2(g) 1 mole of Fe2O3 4 moles of CO 2 moles of Fe 3 moles of CO2
If 1.00 kg of Fe2O3 completely reacts with CO the volume of CO2 released at STP will be?
There are several different possible reactions of Fe2O3 with CO, depending on temperature and ratio of reactants. The simplest is probably Fe2O3 + CO ==>2FeO + CO21.00 Kg x 1000 g/Kg x 1 mole Fe2O3/160 g = 6.25 moles Fe2O3 moles CO2 produced = 6.25 moles CO2 Volume CO2 at STP = 6.25 moles x 22.4 L/mole = 140 Liters
How many moles of CO are produced when 1.4 moles C reacts?
If 1 mole of carbon reacts, 1 mole of CO is produced according to the balanced chemical equation for the reaction. Therefore, if 1.4 moles of carbon react, 1.4 moles of CO will be produced.
How many grams of fe2o3 are required to completely react with 84 grams of co?
160...cant quite grasp HOW though
