I'm having a hard time figuring these out. Please help me on them!
For the reaction Fe2O3 + 3 Co = 2 Fe + 3 CO2:
a) how many moles of Fe can be produced from 75 moles Co?
b) how many moles of CO2 can be produced from 15 moles of Fe2O3?
c) what is the maximum amount (in grams) of CO2 that can be obtained from 454g of Fe2O3?
d) how many grams of CO are needed to react with 275g of Fe2O3?
e) how many grams of CO2 are produced from 195g of CO?
Stoichiometry. All of these are stoichiometry.
a). Look at the equation. The equation TELLS you that 1 mole of Fe2O3 reacts with 3 mols CO (notice that's CO and not Co) to produce 2 mols Fe and 3 mols CO. Therefore, for A, you KNOW from the equation that 3 mols CO will produce 3 mols CO2, so how much CO2 can we get from 75 mols CO?
b. same type problem a a.
c. Convert 454 g Fe2O3 to mols. mols = grams/molar mass. Convert mols Fe2O3 to mols CO2. Then convert mols CO2 to grams CO2.
d. same kind of problem as c.
e. another problem within this one but the same type as c or d.
Post your work if you get stuck.
Your original equation is not balanced. It should be
2 Fe2O3 + 3 Co = 2 Fe + 3 CO2
a) The Fe:Co mole ratio is 2:3
Use that fact to do the calculation
b) The CO2:Fe2O3 mole ratio is 3:2
c) Convert 454 g of Fe2O3 to moles. You will produce 1.5 times as many moles of CO2. Convert that number of moles to grams
d) The CO:Fe2O3 molar ratio is 3:2
e) The CO2:CO molar ratio is 1:1. Use that to get the mass ratio
Someone will be glad to critique your work.
Ignore my answer and go with DrBob's I did not notice that Co should have been CO
To answer these questions, we need to use stoichiometry, which is the calculation of reactants and products in a chemical reaction. The coefficients in the balanced equation provide the ratio of moles between the different substances involved.
a) To determine the moles of Fe produced from 75 moles of Co, we can use the ratio between Co and Fe in the balanced equation.
Given: 75 moles of Co
From the balanced equation: 3 moles of Co react with 2 moles of Fe
Using the ratio, we can set up a proportion:
(75 moles of Co) / (3 moles of Co) = (x moles of Fe) / (2 moles of Fe)
Simplifying the proportion, we find:
x = (75 moles of Co) * (2 moles of Fe) / (3 moles of Co)
x = 50 moles of Fe
Therefore, 75 moles of Co can produce 50 moles of Fe.
b) To determine the moles of CO2 produced from 15 moles of Fe2O3, we will again use the ratio between Fe2O3 and CO2 from the balanced equation.
Given: 15 moles of Fe2O3
From the balanced equation: 1 mole of Fe2O3 reacts with 3 moles of CO2
Setting up the proportion:
(15 moles of Fe2O3) / (1 mole of Fe2O3) = (x moles of CO2) / (3 moles of CO2)
Simplifying the proportion:
x = (15 moles of Fe2O3) * (3 moles of CO2) / (1 mole of Fe2O3)
x = 45 moles of CO2
Therefore, 15 moles of Fe2O3 can produce 45 moles of CO2.
c) To determine the maximum amount of CO2 in grams that can be obtained from 454g of Fe2O3, we first need to convert the given mass of Fe2O3 to moles.
Given: 454g of Fe2O3
Molar mass of Fe2O3 = 159.69 g/mol
Number of moles of Fe2O3 = (454g) / (159.69 g/mol) = 2.84 moles of Fe2O3
From the balanced equation, we know that 1 mole of Fe2O3 produces 3 moles of CO2. So, by multiplying the moles of Fe2O3 by the ratio of CO2 to Fe2O3, we can find the moles of CO2 produced.
Moles of CO2 = (2.84 moles of Fe2O3) * (3 moles of CO2) / (1 mole of Fe2O3) = 8.52 moles of CO2
To convert moles of CO2 to grams, we use the molar mass of CO2.
Molar mass of CO2 = 44.01 g/mol
Grams of CO2 = (8.52 moles of CO2) * (44.01 g/mol) = 375.55 g of CO2
Therefore, the maximum amount of CO2 that can be obtained from 454g of Fe2O3 is 375.55 grams.
d) To determine the grams of CO needed to react with 275g of Fe2O3, we follow a similar process.
Given: 275g of Fe2O3
Molar mass of Fe2O3 = 159.69 g/mol
Number of moles of Fe2O3 = (275g) / (159.69 g/mol) = 1.72 moles of Fe2O3
From the balanced equation, we know that 1 mole of Fe2O3 reacts with 3 moles of CO. So, by multiplying the moles of Fe2O3 by the ratio of CO to Fe2O3, we can find the moles of CO needed.
Moles of CO = (1.72 moles of Fe2O3) * (3 moles of CO) / (1 mole of Fe2O3) = 5.16 moles of CO
To convert moles of CO to grams, we use the molar mass of CO.
Molar mass of CO = 28.01 g/mol
Grams of CO = (5.16 moles of CO) * (28.01 g/mol) = 144.44 g of CO
Therefore, 275g of Fe2O3 would require 144.44 grams of CO.
e) To determine the grams of CO2 produced from 195g of CO, we once again need to convert the given mass of CO to moles.
Given: 195g of CO
Molar mass of CO = 28.01 g/mol
Number of moles of CO = (195g) / (28.01 g/mol) = 6.96 moles of CO
From the balanced equation, we know that 3 moles of CO produce 3 moles of CO2. So, by multiplying the moles of CO by the ratio of CO2 to CO, we can find the moles of CO2 produced.
Moles of CO2 = (6.96 moles of CO) * (3 moles of CO2) / (3 moles of CO) = 6.96 moles of CO2
To convert moles of CO2 to grams, we use the molar mass of CO2.
Molar mass of CO2 = 44.01 g/mol
Grams of CO2 = (6.96 moles of CO2) * (44.01 g/mol) = 306.59 g of CO2
Thus, 195g of CO would produce 306.59 grams of CO2.