so I have this problem and I don't know what numbers to multiple and whatnot. Can someone help me?
This is the problem:
4000 g Fe2O3* 1mole Fe2O3/159.68 gFe2O3* 3mole CO2/1mole Fe2O3
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From what i see your trying to convert 4000 grams of fe203 to moles, and then multiply the find the amount of fe203 in 3 moles of co2. So your answer would be
4000*3/ 159.68
= 75.2 mole of co2 .
now, find how many moles of H2O are there in 45.4 grams H2O?
Of course, I can help you with your problem! It seems like you want to determine the number of moles of carbon dioxide (CO2) produced when 4000 grams of iron(III) oxide (Fe2O3) undergoes a reaction.
To solve this problem, we can use dimensional analysis or the unit conversion method.
First, let's break down the information given in the problem:
- 4000 grams of Fe2O3
- 1 mole of Fe2O3 is equal to 159.68 grams of Fe2O3
- 3 moles of CO2 are produced for every 1 mole of Fe2O3 reacted
Now, let's set up the calculation using dimensional analysis:
Step 1: Start with the given quantity (4000 grams of Fe2O3) and multiply it by the first conversion factor, which is the ratio of moles of Fe2O3 to grams of Fe2O3:
4000 grams Fe2O3 * (1 mole Fe2O3 / 159.68 grams Fe2O3)
Step 2: Next, multiply by the second conversion factor, which is the ratio of moles of CO2 to moles of Fe2O3:
[4000 grams Fe2O3 * (1 mole Fe2O3 / 159.68 grams Fe2O3)] * (3 moles CO2 / 1 mole Fe2O3)
Step 3: Simplify the expression by canceling units:
4000 grams Fe2O3 * (1 mole Fe2O3 / 159.68 grams Fe2O3) * (3 moles CO2 / 1 mole Fe2O3)
The grams of Fe2O3 unit cancels out, leaving us with moles of CO2:
= 4000 * 3 / 159.68 moles CO2 ≈ 75.07 moles CO2
Therefore, approximately 75.07 moles of carbon dioxide are produced when 4000 grams of iron(III) oxide react.