How many grams of Fe2O3 are produced when 17 grams of O2 is reacted?
4 Fe + 3 O2 \rightarrow→ 2 Fe2O3
Answers
Answer:
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Step-by-step explanation:
4 Fe + 3 O2 -->2 Fe2O3
The first question involves a mass of Fe, you will need the molar mass of Fe. [1 mol Fe=55.85 g Fe] The question asks about the moles of O2 but starts with information about Fe, you will need the mole ratio from the balanced chemical equation. [3 mol O2 = 4 mol Fe] Because molar mass is grams per mole and the question starts you with mg, you need the conversion between g and mg.
? moles O2 = 54.3 mg Fe x (10-3 g / 1 mg) x (1 mol Fe/55.85 g) x (3 mol O2 / 4 mol Fe)
(54.3 * 10-3 *1*3)/(1*55.85*4) = 0.1629 / 223.4 = 0.000729 mol O2
How many grams Fe2O3, are produced from the complete reaction of 32.2 g of Fe?
Question asks about grams of Fe2O3; you need the molar mass of iron(III) oxide. [1 mol Fe2O3 = 159.70 g]
Question starts with 32.2 g Fe; you need the molar mass of Fe. [1 mol Fe = 55.85 g]
Question involves both iron and iron(III) oxide; you need the mole ratio from the balanced chemical equation. [4 mol Fe = 2 mol Fe2O3]
?g Fe2O3 = 32.2 g Fe * (1 mol Fe/55.85 g Fe) * (2 mol Fe2O3 / 4 mol Fe)* (159.70 g / 1 mol Fe2O3)
(32.2*1*2*159.7) / (55.85*4*1) = (10248.68) / (223.4) = 46.0 g Fe2O3
Second Type
This problem is only slightly more complicated than your other problem (KClO3)
The balanced reaction is 4Fe + 3O2 = 2Fe2O3
The reason this is a little more complex is that the mole ratios aren't 1:1 like they were in the other problem.
Here are the steps you should take to solve problems like this:
1. Balance the equation (you did that already)
2. Convert what you are given in grams into moles. In this case you'll want to convert 54.3 mg of Fe into moles
3. Find the mole ratio of what you're trying to find (in this case O2) divided by what you are given (in this case Fe).
The mole ratio is simply a fraction using the coefficients from the balanced chemical reaction.
In this case, you want O2 and are given Fe, thus your mole ratio is 3 O2 / 4 Fe
4. Multiply your answer from 2 by your mole ratio in 3 to get moles of what you're trying to find
5. Now you solved the number of moles of what you're trying to find, so convert it back to grams!
Ok so in this problem:
Step 1: done
Step 2: First convert mg to g: 54.3mg Fe = 0.0543g Fe
Now, 0.0543g (1 mol Fe / 55.8g) = 9.73 x 10-4 moles of Fe
Step 3: We found the mole ratio is 3O2/4Fe
Step 4: multiply steps 2 and 3 together: 9.73 x 10-4mol of Fe * 3O2/4Fe = 7.30 x 10-4 mol O2 needed
We don't need to do step 5 because the question wants the number of moles of O2 which is 7.30 x 10-4
To solve the second part, you start with 32.2g of Fe
Step 1: balance... done
Step 2: Convert to moles: 32.2g Fe (1 mol Fe / 55.8g) = 0.577 mol Fe
Step 3: Mole ratio of Fe2O3 to Fe is (2 Fe2O3 / 4 Fe) So the mole ratio is 2/4
Step 4: multiply steps 2 and 3: 0.577 * 2/4 = 0.289 mol Fe2O3 is formed
Step 5: convert product back to grams: 0.289 mol Fe2O3 * ((2*55.8+3*16)grams / 1 mol Fe2O3)
0.289 mol Fe2O3 * ((2*55.8+3*16)grams / 1 mol Fe2O3)
=0.289 * (159.6g) = 46.1 grams of Fe2O3 is produced
Hope this helped!